document_title: Chemical element

question_text: an element or compound which occurs naturally in the earth is a(n)

question_tokens: an element or compound which occurs naturally in the earth is a ( n )

text: Chemical element

text: Description

text: The lightest chemical elements are hydrogen and helium, both created by Big Bang nucleosynthesis during the first 20 minutes of the universe[5] in a ratio of around 3:1 by mass (or 12:1 by number of atoms),[6][7] along with tiny traces of the next two elements, lithium and beryllium. Almost all other elements found in nature were made by various natural methods of nucleosynthesis.[8] On Earth, small amounts of new atoms are naturally produced in nucleogenic reactions, or in cosmogenic processes, such as cosmic ray spallation. New atoms are also naturally produced on Earth as radiogenic daughter isotopes of ongoing radioactive decay processes such as alpha decay, beta decay, spontaneous fission, cluster decay, and other rarer modes of decay.

text: Of the 94 naturally occurring elements, those with atomic numbers 1 through 82 each have at least one stable isotope (except for technetium, element 43 and promethium, element 61, which have no stable isotopes). Isotopes considered stable are those for which no radioactive decay has yet been observed. Elements with atomic numbers 83 through 94 are unstable to the point that radioactive decay of all isotopes can be detected. Some of these elements, notably bismuth (atomic number 83), thorium (atomic number 90), and uranium (atomic number 92), have one or more isotopes with half-lives long enough to survive as remnants of the explosive stellar nucleosynthesis that produced the heavy metals before the formation of our Solar System. At over 1.9×1019 years, over a billion times longer than the current estimated age of the universe, bismuth-209 (atomic number 83) has the longest known alpha decay half-life of any naturally occurring element, and is almost always considered on par with the 80 stable elements.[9][10] The very heaviest elements (those beyond plutonium, element 94) undergo radioactive decay with half-lives so short that they are not found in nature and must be synthesized.

text: As of 2010, there are 118 known elements (in this context, "known" means observed well enough, even from just a few decay products, to have been differentiated from other elements).[11][12] Of these 118 elements, 94 occur naturally on Earth. Six of these occur in extreme trace quantities: technetium, atomic number 43; promethium, number 61; astatine, number 85; francium, number 87; neptunium, number 93; and plutonium, number 94. These 94 elements have been detected in the universe at large, in the spectra of stars and also supernovae, where short-lived radioactive elements are newly being made. The first 94 elements have been detected directly on Earth as primordial nuclides present from the formation of the solar system, or as naturally occurring fission or transmutation products of uranium and thorium.

text: The remaining 24 heavier elements, not found today either on Earth or in astronomical spectra, have been produced artificially: these are all radioactive, with very short half-lives; if any atoms of these elements were present at the formation of Earth, they are extremely likely, to the point of certainty, to have already decayed, and if present in novae, have been in quantities too small to have been noted. Technetium was the first purportedly non-naturally occurring element synthesized, in 1937, although trace amounts of technetium have since been found in nature (and also the element may have been discovered naturally in 1925).[13] This pattern of artificial production and later natural discovery has been repeated with several other radioactive naturally occurring rare elements.[14]

text: List of the elements are available by name, atomic number, density, melting point, boiling point and by symbol, as well as ionization energies of the elements. The nuclides of stable and radioactive elements are also available as a list of nuclides, sorted by length of half-life for those that are unstable. One of the most convenient, and certainly the most traditional presentation of the elements, is in the form of the periodic table, which groups together elements with similar chemical properties (and usually also similar electronic structures).

text: Atomic number

text: The atomic number of an element is equal to the number of protons in each atom, and defines the element.[15] For example, all carbon atoms contain 6 protons in their atomic nucleus; so the atomic number of carbon is 6.[16] Carbon atoms may have different numbers of neutrons; atoms of the same element having different numbers of neutrons are known as isotopes of the element.[17]

text: The number of protons in the atomic nucleus also determines its electric charge, which in turn determines the number of electrons of the atom in its non-ionized state. The electrons are placed into atomic orbitals that determine the atom's various chemical properties. The number of neutrons in a nucleus usually has very little effect on an element's chemical properties (except in the case of hydrogen and deuterium). Thus, all carbon isotopes have nearly identical chemical properties because they all have six protons and six electrons, even though carbon atoms may, for example, have 6 or 8 neutrons. That is why the atomic number, rather than mass number or atomic weight, is considered the identifying characteristic of a chemical element.

text: The symbol for atomic number is Z.

text: Isotopes

text: Isotopes are atoms of the same element (that is, with the same number of protons in their atomic nucleus), but having different numbers of neutrons. Thus, for example, there are three main isotopes of carbon. All carbon atoms have 6 protons in the nucleus, but they can have either 6, 7, or 8 neutrons. Since the mass numbers of these are 12, 13 and 14 respectively, the three isotopes of carbon are known as carbon-12, carbon-13, and carbon-14, often abbreviated to 12C, 13C, and 14C. Carbon in everyday life and in chemistry is a mixture of 12C (about 98.9%), 13C (about 1.1%) and about 1 atom per trillion of 14C.

text: Most (66 of 94) naturally occurring elements have more than one stable isotope. Except for the isotopes of hydrogen (which differ greatly from each other in relative mass—enough to cause chemical effects), the isotopes of a given element are chemically nearly indistinguishable.

text: All of the elements have some isotopes that are radioactive (radioisotopes), although not all of these radioisotopes occur naturally. The radioisotopes typically decay into other elements upon radiating an alpha or beta particle. If an element has isotopes that are not radioactive, these are termed "stable" isotopes. All of the known stable isotopes occur naturally (see primordial isotope). The many radioisotopes that are not found in nature have been characterized after being artificially made. Certain elements have no stable isotopes and are composed only of radioactive isotopes: specifically the elements without any stable isotopes are technetium (atomic number 43), promethium (atomic number 61), and all observed elements with atomic numbers greater than 82.

text: Of the 80 elements with at least one stable isotope, 26 have only one single stable isotope. The mean number of stable isotopes for the 80 stable elements is 3.1 stable isotopes per element. The largest number of stable isotopes that occur for a single element is 10 (for tin, element 50).

text: Isotopic mass and atomic mass

text: The mass number of an element, A, is the number of nucleons (protons and neutrons) in the atomic nucleus. Different isotopes of a given element are distinguished by their mass numbers, which are conventionally written as a superscript on the left hand side of the atomic symbol (e.g. 238U). The mass number is always a whole number and has units of "nucleons". For example, magnesium-24 (24 is the mass number) is an atom with 24 nucleons (12 protons and 12 neutrons).

text: Whereas the mass number simply counts the total number of neutrons and protons and is thus a natural (or whole) number, the atomic mass of a single atom is a real number giving the mass of a particular isotope (or "nuclide") of the element, expressed in atomic mass units (u). In general, the mass number of a given nuclide differs in value slightly from its atomic mass, since the mass of each proton and neutron is not exactly 1 u; since the electrons contribute a lesser share to the atomic mass as neutron number exceeds proton number; and (finally) because of the nuclear binding energy. For example, the atomic mass of chlorine-35 to five significant digits is 34.969 u and that of chlorine-37 is 36.966 u. However, the atomic mass in u of each isotope is quite close to its simple mass number (always within 1%). The only isotope whose atomic mass is exactly a natural number is 12C, which by definition has a mass of exactly 12, because u is defined as 1/12 of the mass of a free neutral carbon-12 atom in the ground state.

text: The standard atomic weight (commonly called "atomic weight") of an element is the average of the atomic masses of all the chemical element's isotopes as found in a particular environment, weighted by isotopic abundance, relative to the atomic mass unit. This number may be a fraction that is not close to a whole number. For example, the relative atomic mass of chlorine is 35.453 u, which differs greatly from a whole number as it is an average of about 76% chlorine-35 and 24% chlorine-37. Whenever a relative atomic mass value differs by more than 1% from a whole number, it is due to this averaging effect, as significant amounts of more than one isotope are naturally present in a sample of that element.

text: Chemically pure and isotopically pure

text: Chemists and nuclear scientists have different definitions of a pure element. In chemistry, a pure element means a substance whose atoms all (or in practice almost all) have the same atomic number, or number of protons. Nuclear scientists, however, define a pure element as one that consists of only one stable isotope.[18]

text: For example, a copper wire is 99.99% chemically pure if 99.99% of its atoms are copper, with 29 protons each. However it is not isotopically pure since ordinary copper consists of two stable isotopes, 69% 63Cu and 31% 65Cu, with different numbers of neutrons. However, a pure gold ingot would be both chemically and isotopically pure, since ordinary gold consists only of one isotope, 197Au.

text: Allotropes

text: Atoms of chemically pure elements may bond to each other chemically in more than one way, allowing the pure element to exist in multiple chemical structures (spatial arrangements of atoms), known as allotropes, which differ in their properties. For example, carbon can be found as diamond, which has a tetrahedral structure around each carbon atom; graphite, which has layers of carbon atoms with a hexagonal structure stacked on top of each other; graphene, which is a single layer of graphite that is very strong; fullerenes, which have nearly spherical shapes; and carbon nanotubes, which are tubes with a hexagonal structure (even these may differ from each other in electrical properties). The ability of an element to exist in one of many structural forms is known as 'allotropy'.

text: The standard state, also known as reference state, of an element is defined as its thermodynamically most stable state at a pressure of 1 bar and a given temperature (typically at 298.15 K). In thermochemistry, an element is defined to have an enthalpy of formation of zero in its standard state. For example, the reference state for carbon is graphite, because the structure of graphite is more stable than that of the other allotropes.

text: Properties

text: Several kinds of descriptive categorizations can be applied broadly to the elements, including consideration of their general physical and chemical properties, their states of matter under familiar conditions, their melting and boiling points, their densities, their crystal structures as solids, and their origins.

text: General properties

text: Several terms are commonly used to characterize the general physical and chemical properties of the chemical elements. A first distinction is between metals, which readily conduct electricity, nonmetals, which do not, and a small group, (the metalloids), having intermediate properties and often behaving as semiconductors.

text: A more refined classification is often shown in colored presentations of the periodic table. This system restricts the terms "metal" and "nonmetal" to only certain of the more broadly defined metals and nonmetals, adding additional terms for certain sets of the more broadly viewed metals and nonmetals. The version of this classification used in the periodic tables presented here includes: actinides, alkali metals, alkaline earth metals, halogens, lanthanides, transition metals, post-transition metals, metalloids, polyatomic nonmetals, diatomic nonmetals, and noble gases. In this system, the alkali metals, alkaline earth metals, and transition metals, as well as the lanthanides and the actinides, are special groups of the metals viewed in a broader sense. Similarly, the polyatomic nonmetals, diatomic nonmetals and the noble gases are nonmetals viewed in the broader sense. In some presentations, the halogens are not distinguished, with astatine identified as a metalloid and the others identified as nonmetals.

text: States of matter

text: Another commonly used basic distinction among the elements is their state of matter (phase), whether solid, liquid, or gas, at a selected standard temperature and pressure (STP). Most of the elements are solids at conventional temperatures and atmospheric pressure, while several are gases. Only bromine and mercury are liquids at 0 degrees Celsius (32 degrees Fahrenheit) and normal atmospheric pressure; caesium and gallium are solids at that temperature, but melt at 28.4 °C (83.2 °F) and 29.8 °C (85.6 °F), respectively.

text: Melting and boiling points

text: Melting and boiling points, typically expressed in degrees Celsius at a pressure of one atmosphere, are commonly used in characterizing the various elements. While known for most elements, either or both of these measurements is still undetermined for some of the radioactive elements available in only tiny quantities. Since helium remains a liquid even at absolute zero at atmospheric pressure, it has only a boiling point, and not a melting point, in conventional presentations.

text: Densities

text: The density at a selected standard temperature and pressure (STP) is frequently used in characterizing the elements. Density is often expressed in grams per cubic centimeter (g/cm3). Since several elements are gases at commonly encountered temperatures, their densities are usually stated for their gaseous forms; when liquefied or solidified, the gaseous elements have densities similar to those of the other elements.

text: When an element has allotropes with different densities, one representative allotrope is typically selected in summary presentations, while densities for each allotrope can be stated where more detail is provided. For example, the three familiar allotropes of carbon (amorphous carbon, graphite, and diamond) have densities of 1.8–2.1, 2.267, and 3.515 g/cm3, respectively.

text: Crystal structures

text: The elements studied to date as solid samples have eight kinds of crystal structures: cubic, body-centered cubic, face-centered cubic, hexagonal, monoclinic, orthorhombic, rhombohedral, and tetragonal. For some of the synthetically produced transuranic elements, available samples have been too small to determine crystal structures.

text: Occurrence and origin on Earth

text: Chemical elements may also be categorized by their origin on Earth, with the first 94 considered naturally occurring, while those with atomic numbers beyond 94 have only been produced artificially as the synthetic products of man-made nuclear reactions.

text: Of the 94 naturally occurring elements, 83 are considered primordial and either stable or weakly radioactive. The remaining 11 naturally occurring elements possess half lives too short for them to have been present at the beginning of the Solar System, and are therefore considered transient elements. Of these 11 transient elements, 5 (polonium, radon, radium, actinium, and protactinium) are relatively common decay products of thorium and uranium. The remaining 6 transient elements (technetium, promethium, astatine, francium, neptunium, and plutonium) occur only rarely, as products of rare decay modes or nuclear reaction processes involving uranium or other heavy elements.

text: Elements with atomic numbers 1 through 40 are all stable, while those with atomic numbers 41 through 82 (except technetium and promethium) are metastable.[citation needed] The half-lives of these metastable "theoretical radionuclides" are so long (at least 100 million times longer than the estimated age of the universe) that their radioactive decay has yet to be detected by experiment. Elements with atomic numbers 83 through 94 are unstable to the point that their radioactive decay can be detected. Three of these elements, bismuth (element 83), thorium (element 90), and uranium (element 92) have one or more isotopes with half-lives long enough to survive as remnants of the explosive stellar nucleosynthesis that produced the heavy elements before the formation of our solar system. For example, at over 1.9×1019 years, over a billion times longer than the current estimated age of the universe, bismuth-209 has the longest known alpha decay half-life of any naturally occurring element.[9][10] The very heaviest 24 elements (those beyond plutonium, element 94) undergo radioactive decay with short half-lives and cannot be produced as daughters of longer-lived elements, and thus they do not occur in nature at all.

text: The periodic table

text:
v
t
e

tag: ul

text:
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

Hydrogen1H7000100800000000000♠1.008

Helium2He7000400260000000000♠4.0026

2
Lithium3Li7000694000000000000♠6.94
Beryllium4Be7000901220000000000♠9.0122

Boron5B7001108100000000000♠10.81
Carbon6C7001120110000000000♠12.011
Nitrogen7N7001140070000000000♠14.007
Oxygen8O7001159990000000000♠15.999
Fluorine9F7001189980000000000♠18.998
Neon10Ne7001201800000000000♠20.180

3
Sodium11Na7001229899999999999♠22.990
Magnesium12Mg7001243050000000000♠24.305

Aluminium13Al7001269820000000000♠26.982
Silicon14Si7001280850000000000♠28.085
Phosphorus15P7001309740000000000♠30.974
Sulfur16S7001320600000000000♠32.06
Chlorine17Cl7001354500000000000♠35.45
Argon18Ar7001399480000000000♠39.948

4
Potassium19K7001390980000000000♠39.098
Calcium20Ca7001400780000000000♠40.078
Scandium21Sc7001449560000000000♠44.956

Titanium22Ti7001478670000000000♠47.867
Vanadium23V7001509420000000000♠50.942
Chromium24Cr7001519960000000000♠51.996
Manganese25Mn7001549380000000000♠54.938
Iron26Fe7001558450000000000♠55.845
Cobalt27Co7001589330000000000♠58.933
Nickel28Ni7001586930000000000♠58.693
Copper29Cu7001635460000000000♠63.546
Zinc30Zn7001653800000000000♠65.38
Gallium31Ga7001697230000000000♠69.723
Germanium32Ge7001726300000000000♠72.630
Arsenic33As7001749220000000000♠74.922
Selenium34Se7001789710000000000♠78.971
Bromine35Br7001799040000000000♠79.904
Krypton36Kr7001837980000000000♠83.798

5
Rubidium37Rb7001854680000000000♠85.468
Strontium38Sr7001876200000000000♠87.62
Yttrium39Y7001889060000000000♠88.906

Zirconium40Zr7001912240000000000♠91.224
Niobium41Nb7001929060000000000♠92.906
Molybdenum42Mo7001959500000000000♠95.95
Technetium43Tc[98]
Ruthenium44Ru7002101070000000000♠101.07
Rhodium45Rh7002102910000000000♠102.91
Palladium46Pd7002106420000000000♠106.42
Silver47Ag7002107870000000000♠107.87
Cadmium48Cd7002112410000000000♠112.41
Indium49In7002114820000000000♠114.82
Tin50Sn7002118710000000000♠118.71
Antimony51Sb7002121760000000000♠121.76
Tellurium52Te7002127600000000000♠127.60
Iodine53I7002126900000000000♠126.90
Xenon54Xe7002131289999999999♠131.29

6
Caesium55Cs7002132910000000000♠132.91
Barium56Ba7002137330000000000♠137.33
Lanthanum57La7002138910000000000♠138.91

Hafnium72Hf7002178490000000000♠178.49
Tantalum73Ta7002180950000000000♠180.95
Tungsten74W7002183840000000000♠183.84
Rhenium75Re7002186210000000000♠186.21
Osmium76Os7002190230000000000♠190.23
Iridium77Ir7002192220000000000♠192.22
Platinum78Pt7002195080000000000♠195.08
Gold79Au7002196970000000000♠196.97
Mercury80Hg7002200590000000000♠200.59
Thallium81Tl7002204380000000000♠204.38
Lead82Pb7002207200000000000♠207.2
Bismuth83Bi7002208980000000000♠208.98
Polonium84Po[209]
Astatine85At[210]
Radon86Rn[222]

7
Francium87Fr[223]
Radium88Ra[226]
Actinium89Ac[227]

Rutherfordium104Rf[267]
Dubnium105Db[268]
Seaborgium106Sg[269]
Bohrium107Bh[270]
Hassium108Hs[270]
Meitnerium109Mt[278]
Darmstadtium110Ds[281]
Roentgenium111Rg[282]
Copernicium112Cn[285]
Nihonium113Nh[286]
Flerovium114Fl[289]
Moscovium115Mc[290]
Livermorium116Lv[293]
Tennessine117Ts[294]
Oganesson118Og[294]

Cerium58Ce7002140120000000000♠140.12
Praseodymium59Pr7002140910000000000♠140.91
Neodymium60Nd7002144240000000000♠144.24
Promethium61Pm[145]
Samarium62Sm7002150360000000000♠150.36
Europium63Eu7002151960000000000♠151.96
Gadolinium64Gd7002157250000000000♠157.25
Terbium65Tb7002158930000000000♠158.93
Dysprosium66Dy7002162500000000000♠162.50
Holmium67Ho7002164930000000000♠164.93
Erbium68Er7002167260000000000♠167.26
Thulium69Tm7002168930000000000♠168.93
Ytterbium70Yb7002173050000000000♠173.05
Lutetium71Lu7002174970000000000♠174.97

Thorium90Th7002232040000000000♠232.04
Protactinium91Pa7002231040000000000♠231.04
Uranium92U7002238030000000000♠238.03
Neptunium93Np[237]
Plutonium94Pu[244]
Americium95Am[243]
Curium96Cm[247]
Berkelium97Bk[247]
Californium98Cf[251]
Einsteinium99Es[252]
Fermium100Fm[257]
Mendelevium101Md[258]
Nobelium102No[259]
Lawrencium103Lr[266]

tag: table

text: 1 (red)=Gas 3 (black)=Solid 80 (green)=Liquid 109 (gray)=Unknown Color of the atomic number shows state of matter (at 0 °C and 1 atm)

text:
Ca: 7001400780000000000♠40.078 — Formal short value, rounded (no uncertainty)[20]
Po: [209] — mass number of the most stable isotope

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

text:
Metal
Metalloid
Nonmetal
Unknown
chemical
properties

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

text: The properties of the chemical elements are often summarized using the periodic table, which powerfully and elegantly organizes the elements by increasing atomic number into rows ("periods") in which the columns ("groups") share recurring ("periodic") physical and chemical properties. The current standard table contains 118 confirmed elements as of 10 April 2010.

text: Although earlier precursors to this presentation exist, its invention is generally credited to the Russian chemist Dmitri Mendeleev in 1869, who intended the table to illustrate recurring trends in the properties of the elements. The layout of the table has been refined and extended over time as new elements have been discovered and new theoretical models have been developed to explain chemical behavior.

text: Use of the periodic table is now ubiquitous within the academic discipline of chemistry, providing an extremely useful framework to classify, systematize and compare all the many different forms of chemical behavior. The table has also found wide application in physics, geology, biology, materials science, engineering, agriculture, medicine, nutrition, environmental health, and astronomy. Its principles are especially important in chemical engineering.

text: Nomenclature and symbols

text: The various chemical elements are formally identified by their unique atomic numbers, by their accepted names, and by their symbols.

text: Atomic numbers

text: The known elements have atomic numbers from 1 through 118, conventionally presented as Arabic numerals. Since the elements can be uniquely sequenced by atomic number, conventionally from lowest to highest (as in a periodic table), sets of elements are sometimes specified by such notation as "through", "beyond", or "from ... through", as in "through iron", "beyond uranium", or "from lanthanum through lutetium". The terms "light" and "heavy" are sometimes also used informally to indicate relative atomic numbers (not densities), as in "lighter than carbon" or "heavier than lead", although technically the weight or mass of atoms of an element (their atomic weights or atomic masses) do not always increase monotonically with their atomic numbers.

text: Element names

text: The naming of various substances now known as elements precedes the atomic theory of matter, as names were given locally by various cultures to various minerals, metals, compounds, alloys, mixtures, and other materials, although at the time it was not known which chemicals were elements and which compounds. As they were identified as elements, the existing names for anciently-known elements (e.g., gold, mercury, iron) were kept in most countries. National differences emerged over the names of elements either for convenience, linguistic niceties, or nationalism. For a few illustrative examples: German speakers use "Wasserstoff" (water substance) for "hydrogen", "Sauerstoff" (acid substance) for "oxygen" and "Stickstoff" (smothering substance) for "nitrogen", while English and some romance languages use "sodium" for "natrium" and "potassium" for "kalium", and the French, Italians, Greeks, Portuguese and Poles prefer "azote/azot/azoto" (from roots meaning "no life") for "nitrogen".

text: For purposes of international communication and trade, the official names of the chemical elements both ancient and more recently recognized are decided by the International Union of Pure and Applied Chemistry (IUPAC), which has decided on a sort of international English language, drawing on traditional English names even when an element's chemical symbol is based on a Latin or other traditional word, for example adopting "gold" rather than "aurum" as the name for the 79th element (Au). IUPAC prefers the British spellings "aluminium" and "caesium" over the U.S. spellings "aluminum" and "cesium", and the U.S. "sulfur" over the British "sulphur". However, elements that are practical to sell in bulk in many countries often still have locally used national names, and countries whose national language does not use the Latin alphabet are likely to use the IUPAC element names.

text: According to IUPAC, chemical elements are not proper nouns in English; consequently, the full name of an element is not routinely capitalized in English, even if derived from a proper noun, as in californium and einsteinium. Isotope names of chemical elements are also uncapitalized if written out, e.g., carbon-12 or uranium-235. Chemical element symbols (such as Cf for californium and Es for einsteinium), are always capitalized (see below).

text: In the second half of the twentieth century, physics laboratories became able to produce nuclei of chemical elements with half-lives too short for an appreciable amount of them to exist at any time. These are also named by IUPAC, which generally adopts the name chosen by the discoverer. This practice can lead to the controversial question of which research group actually discovered an element, a question that delayed the naming of elements with atomic number of 104 and higher for a considerable amount of time. (See element naming controversy).

text: Precursors of such controversies involved the nationalistic namings of elements in the late 19th century. For example, lutetium was named in reference to Paris, France. The Germans were reluctant to relinquish naming rights to the French, often calling it cassiopeium. Similarly, the British discoverer of niobium originally named it columbium, in reference to the New World. It was used extensively as such by American publications prior to the international standardization (in 1950).

text: Chemical symbols

text: Specific chemical elements

text: Before chemistry became a science, alchemists had designed arcane symbols for both metals and common compounds. These were however used as abbreviations in diagrams or procedures; there was no concept of atoms combining to form molecules. With his advances in the atomic theory of matter, John Dalton devised his own simpler symbols, based on circles, to depict molecules.

text: The current system of chemical notation was invented by Berzelius. In this typographical system, chemical symbols are not mere abbreviations—though each consists of letters of the Latin alphabet. They are intended as universal symbols for people of all languages and alphabets.

text: The first of these symbols were intended to be fully universal. Since Latin was the common language of science at that time, they were abbreviations based on the Latin names of metals. Cu comes from Cuprum, Fe comes from Ferrum, Ag from Argentum. The symbols were not followed by a period (full stop) as with abbreviations. Later chemical elements were also assigned unique chemical symbols, based on the name of the element, but not necessarily in English. For example, sodium has the chemical symbol 'Na' after the Latin natrium. The same applies to "W" (wolfram) for tungsten, "Fe" (ferrum) for iron, "Hg" (hydrargyrum) for mercury, "Sn" (stannum) for tin, "K" (kalium) for potassium, "Au" (aurum) for gold, "Ag" (argentum) for silver, "Pb" (plumbum) for lead, "Cu" (cuprum) for copper, and "Sb" (stibium) for antimony.

text: Chemical symbols are understood internationally when element names might require translation. There have sometimes been differences in the past. For example, Germans in the past have used "J" (for the alternate name Jod) for iodine, but now use "I" and "Iod".

text: The first letter of a chemical symbol is always capitalized, as in the preceding examples, and the subsequent letters, if any, are always lower case (small letters). Thus, the symbols for californium and einsteinium are Cf and Es.

text: General chemical symbols

text: There are also symbols in chemical equations for groups of chemical elements, for example in comparative formulas. These are often a single capital letter, and the letters are reserved and not used for names of specific elements. For example, an "X" indicates a variable group (usually a halogen) in a class of compounds, while "R" is a radical, meaning a compound structure such as a hydrocarbon chain. The letter "Q" is reserved for "heat" in a chemical reaction. "Y" is also often used as a general chemical symbol, although it is also the symbol of yttrium. "Z" is also frequently used as a general variable group. "E" is used in organic chemistry to denote an electron-withdrawing group or an electrophile; similarly "Nu" denotes a nucleophile. "L" is used to represent a general ligand in inorganic and organometallic chemistry. "M" is also often used in place of a general metal.

text: At least two additional, two-letter generic chemical symbols are also in informal usage, "Ln" for any lanthanide element and "An" for any actinide element. "Rg" was formerly used for any rare gas element, but the group of rare gases has now been renamed noble gases and the symbol "Rg" has now been assigned to the element roentgenium.

text: Isotope symbols

text: Isotopes are distinguished by the atomic mass number (total protons and neutrons) for a particular isotope of an element, with this number combined with the pertinent element's symbol. IUPAC prefers that isotope symbols be written in superscript notation when practical, for example 12C and 235U. However, other notations, such as carbon-12 and uranium-235, or C-12 and U-235, are also used.

text: As a special case, the three naturally occurring isotopes of the element hydrogen are often specified as H for 1H (protium), D for 2H (deuterium), and T for 3H (tritium). This convention is easier to use in chemical equations, replacing the need to write out the mass number for each atom. For example, the formula for heavy water may be written D2O instead of 2H2O.

text: Origin of the elements

text: Only about 4% of the total mass of the universe is made of atoms or ions, and thus represented by chemical elements. This fraction is about 15% of the total matter, with the remainder of the matter (85%) being dark matter. The nature of dark matter is unknown, but it is not composed of atoms of chemical elements because it contains no protons, neutrons, or electrons. (The remaining non-matter part of the mass of the universe is composed of the even more mysterious dark energy).

text: The universe's 94 naturally occurring chemical elements are thought to have been produced by at least four cosmic processes. Most of the hydrogen and helium in the universe was produced primordially in the first few minutes of the Big Bang. Three recurrently occurring later processes are thought to have produced the remaining elements. Stellar nucleosynthesis, an ongoing process, produces all elements from carbon through iron in atomic number, but little lithium, beryllium, or boron. Elements heavier in atomic number than iron, as heavy as uranium and plutonium, are produced by explosive nucleosynthesis in supernovas and other cataclysmic cosmic events. Cosmic ray spallation (fragmentation) of carbon, nitrogen, and oxygen is important to the production of lithium, beryllium and boron.

text: During the early phases of the Big Bang, nucleosynthesis of hydrogen nuclei resulted in the production of hydrogen-1 (protium, 1H) and helium-4 (4He), as well as a smaller amount of deuterium (2H) and very minuscule amounts (on the order of 10−10) of lithium and beryllium. Even smaller amounts of boron may have been produced in the Big Bang, since it has been observed in some very old stars, while carbon has not.[21] It is generally agreed that no heavier elements than boron were produced in the Big Bang. As a result, the primordial abundance of atoms (or ions) consisted of roughly 75% 1H, 25% 4He, and 0.01% deuterium, with only tiny traces of lithium, beryllium, and perhaps boron.[22] Subsequent enrichment of galactic halos occurred due to stellar nucleosynthesis and supernova nucleosynthesis.[23] However, the element abundance in intergalactic space can still closely resemble primordial conditions, unless it has been enriched by some means.

text: On Earth (and elsewhere), trace amounts of various elements continue to be produced from other elements as products of nuclear transmutation processes. These include some produced by cosmic rays or other nuclear reactions (see cosmogenic and nucleogenic nuclides), and others produced as decay products of long-lived primordial nuclides.[24] For example, trace (but detectable) amounts of carbon-14 (14C) are continually produced in the atmosphere by cosmic rays impacting nitrogen atoms, and argon-40 (40Ar) is continually produced by the decay of primordially occurring but unstable potassium-40 (40K). Also, three primordially occurring but radioactive actinides, thorium, uranium, and plutonium, decay through a series of recurrently produced but unstable radioactive elements such as radium and radon, which are transiently present in any sample of these metals or their ores or compounds. Three other radioactive elements, technetium, promethium, and neptunium, occur only incidentally in natural materials, produced as individual atoms by nuclear fission of the nuclei of various heavy elements or in other rare nuclear processes.

text: Human technology has produced various additional elements beyond these first 94, with those through atomic number 118 now known.

text: Abundance

text: The following graph (note log scale) shows the abundance of elements in our Solar System. The table shows the twelve most common elements in our galaxy (estimated spectroscopically), as measured in parts per million, by mass.[25] Nearby galaxies that have evolved along similar lines have a corresponding enrichment of elements heavier than hydrogen and helium. The more distant galaxies are being viewed as they appeared in the past, so their abundances of elements appear closer to the primordial mixture. As physical laws and processes appear common throughout the visible universe, however, scientist expect that these galaxies evolved elements in similar abundance.

text: The abundance of elements in the Solar System is in keeping with their origin from nucleosynthesis in the Big Bang and a number of progenitor supernova stars. Very abundant hydrogen and helium are products of the Big Bang, but the next three elements are rare since they had little time to form in the Big Bang and are not made in stars (they are, however, produced in small quantities by the breakup of heavier elements in interstellar dust, as a result of impact by cosmic rays). Beginning with carbon, elements are produced in stars by buildup from alpha particles (helium nuclei), resulting in an alternatingly larger abundance of elements with even atomic numbers (these are also more stable). In general, such elements up to iron are made in large stars in the process of becoming supernovas. Iron-56 is particularly common, since it is the most stable element that can easily be made from alpha particles (being a product of decay of radioactive nickel-56, ultimately made from 14 helium nuclei). Elements heavier than iron are made in energy-absorbing processes in large stars, and their abundance in the universe (and on Earth) generally decreases with their atomic number.

text: The abundance of the chemical elements on Earth varies from air to crust to ocean, and in various types of life. The abundance of elements in Earth's crust differs from that in the Solar system (as seen in the Sun and heavy planets like Jupiter) mainly in selective loss of the very lightest elements (hydrogen and helium) and also volatile neon, carbon (as hydrocarbons), nitrogen and sulfur, as a result of solar heating in the early formation of the solar system. Oxygen, the most abundant Earth element by mass, is retained on Earth by combination with silicon. Aluminum at 8% by mass is more common in the Earth's crust than in the universe and solar system, but the composition of the far more bulky mantle, which has magnesium and iron in place of aluminum (which occurs there only at 2% of mass) more closely mirrors the elemental composition of the solar system, save for the noted loss of volatile elements to space, and loss of iron which has migrated to the Earth's core.

text: The composition of the human body, by contrast, more closely follows the composition of seawater—save that the human body has additional stores of carbon and nitrogen necessary to form the proteins and nucleic acids, together with phosphorus in the nucleic acids and energy transfer molecule adenosine triphosphate (ATP) that occurs in the cells of all living organisms. Certain kinds of organisms require particular additional elements, for example the magnesium in chlorophyll in green plants, the calcium in mollusc shells, or the iron in the hemoglobin in vertebrate animals' red blood cells.

text:
Elements in our galaxy
Parts per million
by mass

Hydrogen
739,000

Helium
240,000

Oxygen
10,400

Carbon
4,600

Neon
1,340

Iron
1,090

Nitrogen
960

Silicon
650

Magnesium
580

Sulfur
440

Potassium
210

Nickel
100

text:
Nutritional elements in the periodic table

H

He

Li
Be

B
C
N
O
F
Ne

Na
Mg

Al
Si
P
S
Cl
Ar

K
Ca
Sc

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

Rb
Sr
Y

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

Cs
Ba
La
*
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn

Fr
Ra
Ac
**
Rf
Db
Sg
Bh
Hs
Mt
Ds
Rg
Cn
Nh
Fl
Mc
Lv
Ts
Og

*
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu

**
Th
Pa
U
Np
Pu
Am
Cm
Bk
Cf
Es
Fm
Md
No
Lr

text:
The four basic organic elements

  Quantity elements

  Essential trace elements

  Deemed essential trace element by U.S., not by European Union

  Suggested function from deprivation effects or active metabolic handling, but no clearly-identified biochemical function in humans

  Limited circumstantial evidence for trace benefits or biological action in mammals

  No evidence for biological action in mammals, but essential in some lower organisms.
(In the case of lanthanum, the definition of an essential nutrient as being indispensable and irreplaceable is not completely applicable due to the extreme similarity of the lanthanides. Thus Ce, Pr, and Nd may be substituted for La without ill effects for organisms using La, and the smaller Sm, Eu, and Gd may also be similarly substituted but cause slower growth.)

text: History

text: Evolving definitions

text: The concept of an "element" as an undivisible substance has developed through three major historical phases: Classical definitions (such as those of the ancient Greeks), chemical definitions, and atomic definitions.

text: Classical definitions

text: Ancient philosophy posited a set of classical elements to explain observed patterns in nature. These elements originally referred to earth, water, air and fire rather than the chemical elements of modern science.

text: The term 'elements' (stoicheia) was first used by the Greek philosopher Plato in about 360 BCE in his dialogue Timaeus, which includes a discussion of the composition of inorganic and organic bodies and is a speculative treatise on chemistry. Plato believed the elements introduced a century earlier by Empedocles were composed of small polyhedral forms: tetrahedron (fire), octahedron (air), icosahedron (water), and cube (earth).[26][27]

text: Aristotle, c. 350 BCE, also used the term stoicheia and added a fifth element called aether, which formed the heavens. Aristotle defined an element as:

text: Element – one of those bodies into which other bodies can decompose, and that itself is not capable of being divided into other.[28]

text: Chemical definitions

text: In 1661, Robert Boyle proposed his theory of corpuscularism which favoured the analysis of matter as constituted by irreducible units of matter (atoms) and, choosing to side with neither Aristotle's view of the four elements nor Paracelsus' view of three fundamental elements, left open the question of the number of elements.[29] The first modern list of chemical elements was given in Antoine Lavoisier's 1789 Elements of Chemistry, which contained thirty-three elements, including light and caloric.[30] By 1818, Jöns Jakob Berzelius had determined atomic weights for forty-five of the forty-nine then-accepted elements. Dmitri Mendeleev had sixty-six elements in his periodic table of 1869.

text: From Boyle until the early 20th century, an element was defined as a pure substance that could not be decomposed into any simpler substance.[29] Put another way, a chemical element cannot be transformed into other chemical elements by chemical processes. Elements during this time were generally distinguished by their atomic weights, a property measurable with fair accuracy by available analytical techniques.

text: Atomic definitions

text: The 1913 discovery by English physicist Henry Moseley that the nuclear charge is the physical basis for an atom's atomic number, further refined when the nature of protons and neutrons became appreciated, eventually led to the current definition of an element based on atomic number (number of protons per atomic nucleus). The use of atomic numbers, rather than atomic weights, to distinguish elements has greater predictive value (since these numbers are integers), and also resolves some ambiguities in the chemistry-based view due to varying properties of isotopes and allotropes within the same element. Currently, IUPAC defines an element to exist if it has isotopes with a lifetime longer than the 10−14 seconds it takes the nucleus to form an electronic cloud.[31]

text: By 1914, seventy-two elements were known, all naturally occurring.[32] The remaining naturally occurring elements were discovered or isolated in subsequent decades, and various additional elements have also been produced synthetically, with much of that work pioneered by Glenn T. Seaborg. In 1955, element 101 was discovered and named mendelevium in honor of D.I. Mendeleev, the first to arrange the elements in a periodic manner. Most recently, the synthesis of element 118 was reported in October 2006, and the synthesis of element 117 was reported in April 2010.[33]

text: Discovery and recognition of various elements

text: Ten materials familiar to various prehistoric cultures are now known to be chemical elements: Carbon, copper, gold, iron, lead, mercury, silver, sulfur, tin, and zinc. Three additional materials now accepted as elements, arsenic, antimony, and bismuth, were recognized as distinct substances prior to 1500 AD. Phosphorus, cobalt, and platinum were isolated before 1750.

text: Most of the remaining naturally occurring chemical elements were identified and characterized by 1900, including:

text:
Such now-familiar industrial materials as aluminium, silicon, nickel, chromium, magnesium, and tungsten
Reactive metals such as lithium, sodium, potassium, and calcium
The halogens fluorine, chlorine, bromine, and iodine
Gases such as hydrogen, oxygen, nitrogen, helium, argon, and neon
Most of the rare-earth elements, including cerium, lanthanum, gadolinium, and neodymium.
The more common radioactive elements, including uranium, thorium, radium, and radon

text: Elements isolated or produced since 1900 include:

text:
The three remaining undiscovered regularly occurring stable natural elements: hafnium, lutetium, and rhenium
Plutonium, which was first produced synthetically in 1940 by Glenn T. Seaborg, but is now also known from a few long-persisting natural occurrences
The three incidentally occurring natural elements (neptunium, promethium, and technetium), which were all first produced synthetically but later discovered in trace amounts in certain geological samples
Three scarce decay products of uranium or thorium, (astatine, francium, and protactinium), and
Various synthetic transuranic elements, beginning with americium and curium

text: Recently discovered elements

text: The first transuranium element (element with atomic number greater than 92) discovered was neptunium in 1940. Since 1999 claims for the discovery of new elements have been considered by the IUPAC/IUPAP Joint Working Party. As of January 2016, all 118 elements have been confirmed as discovered by IUPAC. The discovery of element 112 was acknowledged in 2009, and the name copernicium and the atomic symbol Cn were suggested for it.[34] The name and symbol were officially endorsed by IUPAC on 19 February 2010.[35] The heaviest element that is believed to have been synthesized to date is element 118, oganesson, on 9 October 2006, by the Flerov Laboratory of Nuclear Reactions in Dubna, Russia.[12][36] Tennessine, element 117 was the latest element claimed to be discovered, in 2009.[37] On 28 November 2016, scientists at the IUPAC officially recognized the names for four of the newest chemical elements, with atomic numbers 113, 115, 117, and 118.[38][39]

text: List of the 118 known chemical elements

text: The following sortable table shows the 118 known chemical elements.

text:
Atomic number, name, and symbol all serve independently as unique identifiers.
Names are those accepted by IUPAC; provisional names for recently produced elements not yet formally named are in parentheses.
Group, period, and block refer to an element's position in the periodic table. Group numbers here show the currently accepted numbering; for older alternate numberings, see Group (periodic table).
State of matter (solid, liquid, or gas) applies at standard temperature and pressure conditions (STP).
Occurrence, as indicated by a footnote adjacent to the element's name, distinguishes naturally occurring elements, categorized as either primordial or transient (from decay), and additional synthetic elements that have been produced technologically, but are not known to occur naturally.
Color specifies an element's properties using the broad categories commonly presented in periodic tables: Actinide, alkali metal, alkaline earth metal, lanthanide, post-transition metal, metalloid, noble gas, polyatomic or diatomic nonmetal, and transition metal.

text:
[hide]List of chemical elements

Z[I]
Symbol
Element
Origin of name[40][41]
Group
Period
Atomic weight[42][43] (u (±))
Density (g/cm3)
Melt (K) [44]
Boil (K)
C[I] (J/g · K)
χ[I]
Abundance in Earth's crust[II] (mg/kg)

1
H
Hydrogen
composed of the Greek elements hydro- and -gen meaning 'water-forming'
1
1
001 !1.008[III][IV][V][VI]
0.00008988
0014 !14.01
20.28
14.304
2.20
1400

2
He
Helium
the Greek helios, 'sun'
18
1
004 !4.002602(2)[III][V]
0.0001785
0.1 !—[VII]
4.22
5.193
–
0.008

3
Li
Lithium
the Greek lithos, 'stone'
1
2
007 !6.94[III][IV][V][VIII][VI]
0.534
0454 !453.69
1560
3.582
0.98
20

4
Be
Beryllium
beryl, a mineral
2
2
009 !9.0121831(5)
1.85
1560 !1560
2742
1.825
1.57
2.8

5
B
Boron
borax, a mineral
13
2
011 !10.81[III][IV][V][VI]
2.34
2349 !2349
4200
1.026
2.04
10

6
C
Carbon
the Latin carbo, 'coal'
14
2
012 !12.011[III][V][VI]
2.267
3800 !3800
4300
0.709
2.55
200

7
N
Nitrogen
the Greek nitron and '-gen' meaning 'niter-forming'
15
2
014 !14.007[III][V][VI]
0.0012506
0063 !63.15
77.36
1.04
3.04
19

8
O
Oxygen
from the Greek oxy-, both 'sharp' and 'acid', and -gen, meaning 'acid-forming'
16
2
016 !15.999[III][V][VI]
0.001429
0054 !54.36
90.20
0.918
3.44
461000

9
F
Fluorine
the Latin fluere, 'to flow'
17
2
019 !18.998403163(6)
0.001696
0053.5 !53.53
85.03
0.824
3.98
585

10
Ne
Neon
the Greek neos, meaning 'new'
18
2
020 !20.1797(6)[III][IV]
0.0008999
0024.56 !24.56
27.07
1.03
–
0.005

11
Na
Sodium
the English word soda (natrium in Latin)
1
3
023 !22.98976928(2)
0.971
0371 !370.87
1156
1.228
0.93
23600

12
Mg
Magnesium
Magnesia, a district of Eastern Thessaly in Greece
2
3
024 !24.305[VI]
1.738
0923 !923
1363
1.023
1.31
23300

13
Al
Aluminium
from alumina, a compound (originally alumium)
13
3
027 !26.9815385(7)
2.698
0933.5 !933.47
2792
0.897
1.61
82300

14
Si
Silicon
from the Latin silex, 'flint' (originally silicium)
14
3
028 !28.085[V][VI]
2.3296
1687 !1687
3538
0.705
1.9
282000

15
P
Phosphorus
the Greek phoosphoros, 'carrying light'
15
3
031 !30.973761998(5)
1.82
0317.3 !317.30
550
0.769
2.19
1050

16
S
Sulfur
the Latin sulphur, 'fire and brimstone'
16
3
032 !32.06[III][V][VI]
2.067
0388.4 !388.36
717.87
0.71
2.58
350

17
Cl
Chlorine
the Greek chloros, 'greenish yellow'
17
3
035 !35.45[III][IV][V][VI]
0.003214
0171.6 !171.6
239.11
0.479
3.16
145

18
Ar
Argon
the Greek argos, 'idle'
18
3
040 !39.948(1)[III][V]
0.0017837
0083.8 !83.80
87.30
0.52
–
3.5

19
K
Potassium
New Latin potassa, 'potash' (kalium in Latin)
1
4
039 !39.0983(1)
0.862
0336.5 !336.53
1032
0.757
0.82
20900

20
Ca
Calcium
the Latin calx, 'lime'
2
4
041 !40.078(4)[III]
1.54
1115 !1115
1757
0.647
1
41500

21
Sc
Scandium
Scandia, the Latin name for Scandinavia
3
4
045 !44.955908(5)
2.989
1814 !1814
3109
0.568
1.36
22

22
Ti
Titanium
Titans, the sons of the Earth goddess of Greek mythology
4
4
048 !47.867(1)
4.54
1941 !1941
3560
0.523
1.54
5650

23
V
Vanadium
Vanadis, an Old Norse name for the Scandinavian goddess Freyja
5
4
051 !50.9415(1)
6.11
2183 !2183
3680
0.489
1.63
120

24
Cr
Chromium
the Greek chroma, 'color'
6
4
052 !51.9961(6)
7.15
2180 !2180
2944
0.449
1.66
102

25
Mn
Manganese
corrupted from magnesia negra, see Magnesium
7
4
055 !54.938044(3)
7.44
1519 !1519
2334
0.479
1.55
950

26
Fe
Iron
English word (ferrum in Latin)
8
4
056 !55.845(2)
7.874
1811 !1811
3134
0.449
1.83
56300

27
Co
Cobalt
the German word Kobold, 'goblin'
9
4
059 !58.933194(4)
8.86
1768 !1768
3200
0.421
1.88
25

28
Ni
Nickel
from a mischievous sprite of German miner mythology, Nickel
10
4
058 !58.6934(4)
8.912
1728 !1728
3186
0.444
1.91
84

29
Cu
Copper
English word (Latin cuprum)
11
4
064 !63.546(3)[V]
8.96
1357.77
2835
0.385
1.9
60

30
Zn
Zinc
German word Zinke (prong, tooth)
12
4
065 !65.38(2)
7.134
0693 !692.88
1180
0.388
1.65
70

31
Ga
Gallium
Gallia, the Latin name for France
13
4
070 !69.723(1)
5.907
0302.9 !302.9146
2673
0.371
1.81
19

32
Ge
Germanium
Germania, the Latin name for Germany
14
4
073 !72.630(8)
5.323
1211.40
3106
0.32
2.01
1.5

33
As
Arsenic
English word (Latin arsenicum)
15
4
075 !74.921595(6)
5.776
1090 !1090 [IX]
887
0.329
2.18
1.8

34
Se
Selenium
the Greek selene, 'moon'
16
4
079 !78.971(8)[V]
4.809
0453 !453
958
0.321
2.55
0.05

35
Br
Bromine
the Greek bromos, 'stench'
17
4
080 !79.904[VI]
3.122
0265.8 !265.8
332.0
0.474
2.96
2.4

36
Kr
Krypton
the Greek kryptos, 'hidden'
18
4
084 !83.798(2)[III][IV]
0.003733
0115.8 !115.79
119.93
0.248
3
.0001 !1×10−4

37
Rb
Rubidium
the Latin rubidus, 'deep red'
1
5
085 !85.4678(3)[III]
1.532
0312.5 !312.46
961
0.363
0.82
90

38
Sr
Strontium
Strontian, a small town in Scotland
2
5
087 !87.62(1)[III][V]
2.64
1050
1655
0.301
0.95
370

39
Y
Yttrium
Ytterby, Sweden
3
5
089 !88.90584(2)
4.469
1799
3609
0.298
1.22
33

40
Zr
Zirconium
Persian Zargun, 'gold-colored'; German Zirkoon, 'jargoon'
4
5
091 !91.224(2)[III]
6.506
2128
4682
0.278
1.33
165

41
Nb
Niobium
Niobe, daughter of king Tantalus from Greek mythology
5
5
093 !92.90637(2)
8.57
2750
5017
0.265
1.6
20

42
Mo
Molybdenum
the Greek molybdos meaning 'lead'
6
5
096 !95.95(1)[III]
10.22
2896
4912
0.251
2.16
1.2

43
Tc
Technetium
the Greek tekhnètos meaning 'artificial'
7
5
098 ![98][X]
11.5
2430
4538
–
1.9
.000000003 !~ 3×10−9[XI]

44
Ru
Ruthenium
Ruthenia, the New Latin name for Russia
8
5
101.07(2)[III]
12.37
2607
4423
0.238
2.2
0.001

45
Rh
Rhodium
the Greek rhodos, meaning 'rose coloured'
9
5
102.90550(2)
12.41
2237
3968
0.243
2.28
0.001

46
Pd
Palladium
the then recently discovered asteroid Pallas, considered a planet at the time
10
5
106.42(1)[III]
12.02
1828.05
3236
0.244
2.2
0.015

47
Ag
Silver
English word (argentum in Latin)
11
5
107.8682(2)[III]
10.501
1234.93
2435
0.235
1.93
0.075

48
Cd
Cadmium
the New Latin cadmia, from King Kadmos
12
5
112.414(4)[III]
8.69
0594.22 !594.22
1040
0.232
1.69
0.159

49
In
Indium
indigo
13
5
114.818(1)
7.31
0429.75 !429.75
2345
0.233
1.78
0.25

50
Sn
Tin
English word (stannum in Latin)
14
5
118.710(7)[III]
7.287
0505.08 !505.08
2875
0.228
1.96
2.3

51
Sb
Antimony
uncertain: perhaps from the Greek anti, 'against', and monos, 'alone', or the Old French antimoine, 'Monk's bane' (stibium in Latin)
15
5
121.760(1)[III]
6.685
0903.78 !903.78
1860
0.207
2.05
0.2

52
Te
Tellurium
Latin tellus, 'earth'
16
5
127.60(3)[III]
6.232
0722.66 !722.66
1261
0.202
2.1
0.001

53
I
Iodine
French iode (after the Greek ioeides, 'violet')
17
5
126.90447(3)
4.93
0386.85 !386.85
457.4
0.214
2.66
0.45

54
Xe
Xenon
the Greek xenos, 'strange'
18
5
131.293(6)[III][IV]
0.005887
0161.4 !161.4
165.03
0.158
2.6
.00003 !3×10−5

55
Cs
Caesium
the Latin caesius, 'sky blue'
1
6
132.90545196(6)
1.873
0301.59 !301.59
944
0.242
0.79
3

56
Ba
Barium
the Greek barys, 'heavy'
2
6
137.327(7)
3.594
1000
2170
0.204
0.89
425

57
La
Lanthanum
the Greek lanthanein, 'to lie hidden'
3
6
138.90547(7)[III]
6.145
1193
3737
0.195
1.1
39

58
Ce
Cerium
the then recently discovered asteroid Ceres, considered a planet at the time

6
140.116(1)[III]
6.77
1068
3716
0.192
1.12
66.5

59
Pr
Praseodymium
the Greek praseios didymos meaning 'green twin'

6
140.90766(2)
6.773
1208
3793
0.193
1.13
9.2

60
Nd
Neodymium
the Greek neos didymos meaning 'new twin'

6
144.242(3)[III]
7.007
1297
3347
0.19
1.14
41.5

61
Pm
Promethium
Prometheus of Greek mythology who stole fire from the Gods and gave it to humans

6
145 ![145][X]
7.26
1315
3273
–
1.13
.0000000000000000002 !2×10−19[XI]

62
Sm
Samarium
Samarskite, the name of the mineral from which it was first isolated

6
150.36(2)[III]
7.52
1345
2067
0.197
1.17
7.05

63
Eu
Europium
Europe

6
151.964(1)[III]
5.243
1099
1802
0.182
1.2
2

64
Gd
Gadolinium
Johan Gadolin, chemist, physicist and mineralogist

6
157.25(3)[III]
7.895
1585
3546
0.236
1.2
6.2

65
Tb
Terbium
Ytterby, Sweden

6
158.92535(2)
8.229
1629
3503
0.182
1.2
1.2

66
Dy
Dysprosium
the Greek dysprositos, 'hard to get'

6
162.500(1)[III]
8.55
1680
2840
0.17
1.22
5.2

67
Ho
Holmium
Holmia, the New Latin name for Stockholm

6
164.93033(2)
8.795
1734
2993
0.165
1.23
1.3

68
Er
Erbium
Ytterby, Sweden

6
167.259(3)[III]
9.066
1802
3141
0.168
1.24
3.5

69
Tm
Thulium
Thule, the ancient name for Scandinavia

6
168.93422(2)
9.321
1818
2223
0.16
1.25
0.52

70
Yb
Ytterbium
Ytterby, Sweden

6
173.045(10)[III]
6.965
1097
1469
0.155
1.1
3.2

71
Lu
Lutetium
Lutetia, the Latin name for Paris

6
174.9668(1)[III]
9.84
1925
3675
0.154
1.27
0.8

72
Hf
Hafnium
Hafnia, the New Latin name for Copenhagen
4
6
178.49(2)
13.31
2506
4876
0.144
1.3
3

73
Ta
Tantalum
King Tantalus, father of Niobe from Greek mythology
5
6
180.94788(2)
16.654
3290
5731
0.14
1.5
2

74
W
Tungsten
the Swedish tung sten, 'heavy stone' (W is wolfram, the old name of the tungsten mineral wolframite)
6
6
183.84(1)
19.25
3695
5828
0.132
2.36
1.3

75
Re
Rhenium
Rhenus, the Latin name for the river Rhine
7
6
186.207(1)
21.02
3459
5869
0.137
1.9
.0007 !7×10−4

76
Os
Osmium
the Greek osmè, meaning 'smell'
8
6
190.23(3)[III]
22.61
3306
5285
0.13
2.2
0.002

77
Ir
Iridium
Iris, the Greek goddess of the rainbow
9
6
192.217(3)
22.56
2719
4701
0.131
2.2
0.001

78
Pt
Platinum
the Spanish platina, meaning 'little silver'
10
6
195.084(9)
21.46
2041.4
4098
0.133
2.28
0.005

79
Au
Gold
English word (aurum in Latin)
11
6
196.966569(5)
19.282
1337.33
3129
0.129
2.54
0.004

80
Hg
Mercury
the New Latin name mercurius, named after the Roman god (Hg from former name hydrargyrum, from Greek hydr-, 'water', and argyros, 'silver')
12
6
200.592(3)
13.5336
0234.43 !234.43
629.88
0.14
2
0.085

81
Tl
Thallium
the Greek thallos, 'green twig'
13
6
204.38[VI]
11.85
0577 !577
1746
0.129
1.62
0.85

82
Pb
Lead
English word (plumbum in Latin)
14
6
207.2(1)[III][V]
11.342
0600.61 !600.61
2022
0.129
1.87
14

83
Bi
Bismuth
Uncertain, possibly Arabic or German
15
6
208.98040(1)[X]
9.807
0544.7 !544.7
1837
0.122
2.02
0.009

84
Po
Polonium
Named after the home country of Marie Curie (Polonia, Latin for Poland), who is also the discoverer of Radium
16
6
209 ![209][X]
9.32
0527 !527
1235
–
2.0
.0000000002 !2×10−10[XI]

85
At
Astatine
the Greek astatos, 'unstable'
17
6
210 ![210][X]
7
0575 !575
610
–
2.2
0.000000000000000000003 !3×10−20[XI]

86
Rn
Radon
From radium, as it was first detected as an emission from radium during radioactive decay
18
6
222 ![222][X]
0.00973
0202 !202
211.3
0.094
2.2
.0000000000004 !4×10−13[XI]

87
Fr
Francium
Francia, the New Latin name for France
1
7
223 ![223][X]
1.87
0300 !300
950
–
0.7
0.000000000000000001 !~ 1×10−18[XI]

88
Ra
Radium
the Latin radius, 'ray'
2
7
223 ![226][X]
5.5
0973 !973
2010
0.094
0.9
.0000009 !9×10−7[XI]

89
Ac
Actinium
the Greek aktis, 'ray'
3
7
227 ![227][X]
10.07
1323
3471
0.12
1.1
.00000000055 !5.5×10−10[XI]

90
Th
Thorium
Thor, the Scandinavian god of thunder

7
232.0377(4)[X][III]
11.72
2115
5061
0.113
1.3
9.6

91
Pa
Protactinium
the Greek protos, 'first', and actinium, which is produced through the radioactive decay of protactinium

7
231.03588(2)[X]
15.37
1841
4300
–
1.5
.0000014 !1.4×10−6[XI]

92
U
Uranium
Uranus, the seventh planet in the Solar System

7
238.02891(3)[X]
18.95
1405.3
4404
0.116
1.38
2.7

93
Np
Neptunium
Neptune, the eighth planet in the Solar System

7
237 ![237][X]
20.45
0917 !917
4273
–
1.36
0.000000000003 !≤ 3×10−12[XI]

94
Pu
Plutonium
Pluto, a dwarf planet in the Solar System (then considered the ninth planet)

7
244 ![244][X]
19.84
0912.5 !912.5
3501
–
1.28
0.00000000003 !≤ 3×10−11[XI]

95
Am
Americium
The Americas, as the element was first synthesized on the continent, by analogy with europium

7
243 ![243][X]
13.69
1449
2880
–
1.13
0 !0[XII]

96
Cm
Curium
Pierre Curie, a physicist, and Marie Curie, a physicist and chemist, named after great scientists by analogy with gadolinium

7
247 ![247][X]
13.51
1613
3383
–
1.28
0 !0[XII]

97
Bk
Berkelium
Berkeley, California, where the element was first synthesized, by analogy with terbium

7
247 ![247][X]
14.79
1259
2900
–
1.3
0 !0[XII]

98
Cf
Californium
California, where the element was first synthesized

7
251 ![251][X]
15.1
1173
1743 !(1743)[XIII]
–
1.3
0 !0[XII]

99
Es
Einsteinium
Albert Einstein, physicist

7
252 ![252][X]
8.84
1133
1269 !(1269)[XIII]
–
1.3
0 !0[XII]

100
Fm
Fermium
Enrico Fermi, physicist

7
257 ![257][X]
9.7 !(9.7)[XIII]
1125 !(1125)[XIII]
–
–
1.3
0 !0[XII]

101
Md
Mendelevium
Dmitri Mendeleev, chemist and inventor

7
258 ![258][X]
10.3 !(10.3)[XIII]
1100 !(1100)[XIII]
–
–
1.3
0 !0[XII]

102
No
Nobelium
Alfred Nobel, chemist, engineer, innovator, and armaments manufacturer

7
259 ![259][X]
9.9 !(9.9)[XIII]
1100 !(1100)[XIII]
–
–
1.3
0 !0[XII]

103
Lr
Lawrencium
Ernest O. Lawrence, physicist

7
266 ![266][X]
15.6 !(15.6)[XIII]
1900 !(1900)[XIII]
–
–
1.3
0 !0[XII]

104
Rf
Rutherfordium
Ernest Rutherford, chemist and physicist
4
7
267 ![267][X]
23.2 !(23.2)[XIII]
2400 !(2400)[XIII]
5800 !(5800)[XIII]
–
–
0 !0[XII]

105
Db
Dubnium
Dubna, Russia
5
7
268 ![268][X]
29.3 !(29.3)[XIII]
–
–
–
–
0 !0[XII]

106
Sg
Seaborgium
Glenn T. Seaborg, scientist
6
7
269 ![269][X]
35.0 !(35.0)[XIII]
–
–
–
–
0 !0[XII]

107
Bh
Bohrium
Niels Bohr, physicist
7
7
270 ![270][X]
37.1 !(37.1)[XIII]
–
–
–
–
0 !0[XII]

108
Hs
Hassium
Hesse, Germany, where the element was first synthesized
8
7
277 ![277][X]
40.7 !(40.7)[XIII]
–
–
–
–
0 !0[XII]

109
Mt
Meitnerium
Lise Meitner, physicist
9
7
278 ![278][X]
37.4 !(37.4)[XIII]
–
–
–
–
0 !0[XII]

110
Ds
Darmstadtium
Darmstadt, Germany, where the element was first synthesized
10
7
281 ![281][X]
34.8 !(34.8)[XIII]
–
–
–
–
0 !0[XII]

111
Rg
Roentgenium
Wilhelm Conrad Röntgen, physicist
11
7
282 ![282][X]
28.7 !(28.7)[XIII]
–
–
–
–
0 !0[XII]

112
Cn
Copernicium
Nicolaus Copernicus, astronomer
12
7
285 ![285][X]
23.7 !(23.7)[XIII]
–
357 !~357[XIV]
–
–
0 !0[XII]

113
Nh
Nihonium
the Japanese name for Japan, Nihon, where the element was first synthesized
13
7
286 ![286][X]
16 !(16)[XIII]
0700 !(700)[XIII]
1400 !(1400)[XIII]
–
–
0 !0[XII]

114
Fl
Flerovium
Flerov Laboratory of Nuclear Reactions, part of JINR where the element was synthesized; itself named for Georgy Flyorov, physicist
14
7
289 ![289][X]
14 !(14)[XIII]
–
210 !~210
–
–
0 !0[XII]

115
Mc
Moscovium
Moscow Oblast, Russia, where the element was first synthesized
15
7
290 ![290][X]
13.5 !(13.5)[XIII]
0700 !(700)[XIII]
1400 !(1400)[XIII]
–
–
0 !0[XII]

116
Lv
Livermorium
Lawrence Livermore National Laboratory (in Livermore, California) which collaborated with JINR on its synthesis
16
7
293 ![293][X]
12.9 !(12.9)[XIII]
0709 !(709)[XIII]
1085 !(1085)[XIII]
–
–
0 !0[XII]

117
Ts
Tennessine
Tennessee, United States
17
7
294 ![294][X]
7.2 !(7.2)[XIII]
0723 !(723)[XIII]
0883 !(883)[XIII]
–
–
0 !0[XII]

118
Og
Oganesson
Yuri Oganessian, physicist
18
7
294 ![294][X]
5.0 !(5.0)[XIII][XV]
–
350 !(350)[XIII]
–
–
0 !0[XII]

[show]
Notes

^ Jump up to: a b c Z is the standard symbol for atomic number; C is the standard symbol for heat capacity; and χ is the standard symbol for electronegativity on the Pauling scale.
Jump up ^ Unless otherwise indicated, elements are primordial – they occur naturally, and not through decay.
^ Jump up to: a b c d e f g h i j k l m n o p q r s t u v w x y z aa ab ac ad ae af ag ah ai aj ak al The isotopic composition of this element varies in some geological specimens, and the variation may exceed the uncertainty stated in the table.
^ Jump up to: a b c d e f g The isotopic composition of the element can vary in commercial materials, which can cause the atomic weight to deviate significantly from the given value.
^ Jump up to: a b c d e f g h i j k l m n o The isotopic composition varies in terrestrial material such that a more precise atomic weight can not be given.
^ Jump up to: a b c d e f g h i j k l The value listed is the conventional atomic-weight value suitable for trade and commerce. The actual value may differ depending on the isotopic composition of the sample. Since 2009, IUPAC provides the standard atomic-weight values for these elements using the interval notation. The corresponding standard atomic weights are:

Hydrogen: [1.00784, 1.00811]
Lithium: [6.938, 6.997]
Boron: [10.806, 10.821]
Carbon: [12.0096, 12.0116]
Nitrogen: [14.00643, 14.00728]
Oxygen: [15.99903, 15.99977]
Magnesium: [24.304, 24.307]
Silicon: [28.084, 28.086]
Sulfur: [32.059, 32.076]
Chlorine: [35.446, 35.457]
Bromine: [79.901, 79.907]
Thallium: [204.382, 204.385]

Jump up ^ This element does not solidify at a pressure of one atmosphere. Helium can only solidify at pressures above 25 atmospheres, which corresponds to a melting point of absolute zero.
Jump up ^ The atomic weight of commercial lithium can vary between 6.939 and 6.996—analysis of the specific material is necessary to find a more accurate value.
Jump up ^ This element sublimes at one atmosphere of pressure.
^ Jump up to: a b c d e f g h i j k l m n o p q r s t u v w x y z aa ab ac ad ae af ag ah ai aj ak al The element does not have any stable nuclides, and a value in brackets, e.g. [209], indicates the mass number of the longest-lived isotope of the element. However, four such elements, bismuth, thorium, protactinium, and uranium, have characteristic terrestrial isotopic compositions, and thus their standard atomic weights are given.
^ Jump up to: a b c d e f g h i j k This element is transient – it occurs only through decay.
^ Jump up to: a b c d e f g h i j k l m n o p q r s t u v w x This element is synthetic – the transuranic elements 95 and above do not occur naturally, but they can all be produced artificially.
^ Jump up to: a b c d e f g h i j k l m n o p q r s t u v w x y z aa ab ac ad ae af ag ah ai aj The value has not been precisely measured, usually because of the element's short half-life; the value given in parentheses is a prediction.
Jump up ^ With error bars: 357+112
−108 K.
Jump up ^ This predicted value is for liquid oganesson, not gaseous oganesson.


document_title: Made in America (The Sopranos)

question_text: what ballad was featured in the last episode of the sopranos

root

text: Made in America (The Sopranos)

text: Starring[edit]

text:
James Gandolfini as Tony Soprano
Lorraine Bracco as Dr. Jennifer Melfi *
Edie Falco as Carmela Soprano
Michael Imperioli as Christopher Moltisanti **
Dominic Chianese as Corrado "Junior" Soprano
Steven Van Zandt as Silvio Dante
Tony Sirico as Paulie Gualtieri
Robert Iler as Anthony Soprano, Jr.
Jamie-Lynn Sigler as Meadow Soprano
Aida Turturro as Janice Soprano Baccalieri
Frank Vincent as Phil Leotardo
Ray Abruzzo as Little Carmine Lupertazzi
Dan Grimaldi as Patsy Parisi
Sharon Angela as Rosalie Aprile
Maureen Van Zandt as Gabriella Dante

text: * = credit only ** = photo only

tag: p

text: Guest starring[edit]

text:
Gregory Antonacci as Butch DeConcini
Max Casella as Benny Fazio
Carl Capotorto as "Little Paulie" Germani
Arthur J. Nascarella as Carlo Gervasi
Matt Servitto as Agent Harris
Frank Albanese as Patrizio "Uncle Pat" Blundetto
John Cenatiempo as Anthony Maffei
John "Cha Cha" Ciarcia as Albie Cianflone
Michele DeCesare as Hunter Scangarelo
Michael Drayer as Jason Parisi
Frank John Hughes as Walden Belfiore
Michael Kelly as Agent Goddard
Geraldine LiBrandi as Patty Leotardo
David Margulies as Neil Mink
Angelo Massagli as Bobby Baccalieri, Jr.
Peter Mele as George Paglieri
Donna Pescow as Donna Parisi
Joseph Perrino as Jason Gervasi
Anthony Ribustello as Dante Greco
Daniel Sauli as Patrick Parisi
Jenna Stern as Dr. Doherty
Emily Wickersham as Rhiannon Flammer
Danielle Di Vecchio as Barbara Soprano Giglione
Ed Vassallo as Tom Giglione
Ricky Aiello as Raymond "Ray-Ray" D'Abaldo
Melanie Minichino as Tara Zincone
Amy Russ as Female FBI Agent
Paolo Colandrea as Man in Members Only Jacket
Rajesh Bose as Gas Station Manager
Avery Elaine and Emily Ruth Pulcher as Domenica Baccalieri (photo only)

text: Plot summary[edit]

text: Tony is in hiding with his crew. At nightfall, he meets FBI Agent Harris and gives him information about Ahmed and Muhammad. In exchange, he asks for Phil's location, but Harris says he knows nothing. Tony visits his family in the safe house where they are hiding and later joins them in attending Bobby's funeral. Tony visits Janice at her house; she tells him she will raise Bobby's children. Harris calls Tony with information that Phil has been using payphones from gas stations in Oyster Bay, Long Island, and Tony's crew begins surveilling gas stations in the area.

text: Phil calls Butchie from a payphone, expresses anger about his failure to kill Tony, and rejects Butchie's suggestion to make peace. Tony meets with Butchie to negotiate without Phil's knowledge. Butchie refuses to disclose his boss' location, but agrees to a truce and tells Tony to "do what you gotta do".

text: Tony and his family move back into their North Caldwell home. Benny and Walden track Phil to a gas station and shoot him dead; Agent Harris is pleased by this news, seemingly because there was an FBI pool on which crime family would kill the other.

text: A.J. and his girlfriend Rhiannon escape from his SUV after he left its engine running in dry leaves and let it catch fire. He takes up jogging and tells his parents he intends to join the Army. They arrange for him to work for Little Carmine's film production company, instead.

text: Meadow and Patrick announce they are engaged and that Meadow may land a job at a law firm. Meadow tells Tony she wants to defend those oppressed by the government, particularly immigrants; she considers her father a victim of FBI prejudice against Italian-Americans. Tony visits the comatose Silvio in the hospital.

text: Carlo goes missing; Paulie fears he may have become an informant after his son Jason was arrested on a drugs charge. Tony's lawyer, Neil Mink, tells Tony that Carlo is likely testifying and that Tony will be indicted.

text: With Carlo gone, Tony offers the leadership of the Aprile crew to Paulie. Paulie initially refuses, worrying that the crew is cursed, but accepts when Tony tells him he will offer the position to Patsy.

text: Janice meets Junior in the care home to tell him of Bobby's death, but Junior is too confused to understand. Pat tells Tony he believes Janice is scheming to claim for herself the last money Junior's accountant is holding.

text: Tony visits Junior and tells him to give the money to Bobby's children, but realizes Junior does not recognize him. Junior reacts with surprise when Tony reminds him of his involvement in the Mafia, and Tony leaves with tears in his eyes.

text: The Sopranos arrange to meet at a diner. Tony arrives first, and watches customers come and go. Carmela arrives next, and Tony tells her Carlo will testify. A.J. then arrives and reminds his father of his advice to "remember the good times". Meadow arrives late and parks her car outside. As the bell rings, Tony looks up.

text: Production[edit]

text: Conception[edit]

text: Showrunner David Chase planned the series ending and the final scene during the 21-month hiatus between Seasons 5 and 6, a long break HBO had granted him. The final scene was filmed almost exactly as Chase had envisioned. It was not intended as a setup for a future film, although Chase later commented "[t]here may be a day where we all come up with something," regarding a possible Sopranos feature. It was then-HBO chairman Chris Albrecht who suggested to Chase to conclude the series with the sixth season.[1][2][3]

text: Writing[edit]

text: As with every episode of the season, the plot outline of "Made in America" was developed by Chase and his writing staff, which for the final season consisted of executive producers Terence Winter and Matthew Weiner, and supervising producers and writing team Diane Frolov and Andrew Schneider. Frequent episode director Tim Van Patten also provided Chase with some storyline suggestions.[4][5] After the episode's story had been outlined, Chase wrote the first draft. After some input from his writing staff, Chase revised the script to its finished state, although he also made minor changes during filming. "Made in America" is Chase's 30th and final official writing credit (including story credits) for the series and his ninth as sole writer of an episode.[6][7]

text: Chase included allusions to real-life American Mafia history and events in the script for "Made in America", something he is well known for.[6] Specifically, the line "Damn! We're gonna win this thing!", spoken in the episode by the character Dwight Harris after being informed of the death of Phil Leotardo, alludes to former FBI supervisor Lindley DeVecchio. DeVecchio famously uttered the line after being told that Lorenzo "Larry" Lampasi had been shot to death in front of his Brooklyn home and was later charged for informing the Mafia on various accounts, another parallel to Tony Soprano and Dwight Harris.[1][8][9]

text: Cast notes[edit]

text: Maureen Van Zandt, who plays Gabriella Dante, is promoted to the main cast and billed in the opening credits but for this episode only. She is the final addition to the main cast of The Sopranos.

text: Filming[edit]

text: "Made in America" was directed by Chase and photographed by Alik Sakharov. The two served in the same capacities for the pilot episode, "The Sopranos", which was filmed in 1997. The series finale marks the second time Chase has officially directed an episode of The Sopranos, although as showrunner, he would oversee the direction of most episodes throughout the show's production.[10] "Made in America" marks the 38th and final credit for Sakharov as director of photography.

text: Principal photography commenced in late February and concluded in late March 2007. Exterior scenes and certain interior scenes of "Made in America" were filmed on location in Bergen County, New Jersey and in Brooklyn and Manhattan, New York City, New York. Additional interior scenes—including indoor shots of the Soprano residence and the back room of the strip club Bada Bing!—were filmed in a sound stage in Silvercup Studios, New York, where most such scenes of the series had been filmed. The final scene of the episode was filmed in late March 2007 at Holsten's Brookdale Confectionery, an ice cream and candy shop located in Bloomfield, New Jersey. The Bloomfield Township Council initially tried to stop HBO from filming in the town because "[they] found the HBO mob drama offensive to Italian-Americans" and voted to deny the production company a filming permit. However, as the council had no authority to stop filming in the town as long as the crew met the requirements stated in Bloomfield's code for filming crews, a permit was later issued.[11][12] As the show's producers needed to ensure that plot details of the ending would be kept a secret until the airdate, the scripts given to the crew members had their final pages removed. The final scene of these edited scripts was the one in which Tony is raking leaves outside his house, a scene that occurs 10 minutes before the real ending in the final cut. Chase received compliments for this scene from people who thought it was the real ending.[6][13]

text: Post-production[edit]

text: "Made in America" was edited by Sidney Wolinsky, one of the show's three editors, under the supervision of Chase.[10] Chase originally wanted the black screen at the end of the episode to last "all the way to the HBO whoosh sound," meaning that no credits would roll at the end of the episode, but did not receive a waiver from the Directors Guild of America to do so.[14][15]

text: Music[edit]

text: "Don't Stop Believin'" is played throughout the final scene of the series. Journey's lead singer Steve Perry initially refused to let David Chase use the song until he knew the fate of the leading characters and did not give final approval until three days before the episode aired. Perry feared that the song would be remembered as the soundtrack to Tony's demise until Chase assured him that would not be the case.[16] Immediately following the airing of "Made in America," the song enjoyed a great surge of popularity; its sales on iTunes, for example, grew 482 percent.[17] The newly growing attention to the band helped it climb out of the reportedly difficult times it was having at the time.[18]

text: Interpretations of the final scene[edit]

text: The final scene of "Made in America" became the subject of much discussion, controversy, and analysis after its original broadcast. The use of an abrupt cut to black followed by several seconds of silence led many viewers to initially believe that their cable or DVR had cut out at a crucial moment.[19] Opposing interpretations soon emerged among viewers regarding the ultimate fate of series protagonist Tony Soprano, with some believing that he was killed while others believe that he remains alive.[1][20]

text: One argument for the former points to a conversation that Tony had in the midseason premiere episode "Soprano Home Movies" with his brother-in-law Bobby, in which Bobby comments on how suddenly and without sound death can happen in their lives as gangsters: "You probably don't even hear it when it happens, right?" A flashback to this scene also appears in the final minutes of "The Blue Comet", the episode preceding "Made in America".[21][22] When questioned on the theory, HBO spokesman Quentin Schaffer stated that the conversation is a "legitimate" hint.[20] Also, Butchie DeConcini (the presumed successor of Phil Leotardo) was last seen saddled with reparations following the mob war. He had expressed ideas about killing Tony before ("Kaisha"), and Tony was, in the end, the very last DiMeo man left standing out of the three original Lupertazzi targets, who, Phil believed, if killed, would totally cripple the Jersey family. Hence, Tony would have been a tempting target of a hit. The final scene showing a man who glances at Tony (credited as "Man in Members Only Jacket") and who later goes to the bathroom, has been interpreted as a nod to the famous scene in The Godfather in which Michael Corleone retrieves a gun from the bathroom before shooting his enemies to death (Tony's favorite scene from the film, as revealed in the episode "Johnny Cakes").[23] Speculation has also linked the jacket of the man to the title of the opening episode of the season, "Members Only", in which Tony is shot, and also as a symbolic reference to the mysterious man's membership of the Mafia. Actor Matt Servitto said that in the script, the scene continued with the man in the Members Only jacket emerging from the bathroom and starting to walk towards Tony's table.[24] Servitto later clarified this statement, saying that he did not mean to imply that there was a completely different scripted ending, only that the "genius" editing was not what he had expected.[25]

text: Other viewers offer opposing interpretations. It has been suggested that the final scene portrays that, while Tony's life is fraught with fear and danger, which could come from anyone anywhere, and that while Tony has to constantly watch his back and look out for any emerging trouble (he keeps an eye on the diner entrance), life nevertheless goes on and the viewer simply does not get to continue seeing it. The lyrics of the closing song, seemingly telling the viewer "Don't stop believin'," are thought to support this, while the silent black screen space before the credits is meant to allow people to imagine and believe in their own continuations of Tony's story.[26] It can be stated that because of Tony's peace agreement with the Lupertazzi family, their tacit sanction of a hit on Phil, and Butchie's visible unwillingness to continue the hostilities, there was little legitimate basis to expect a hit on Tony from the Lupertazzis and the threat to him, although always present, was not higher than usual.[27]

text: Comments from David Chase[edit]

text: Chase has made various comments about the finale but has avoided providing an explanation to the meaning of the final scene. In his first interview after the broadcast of the finale with New Jersey paper The Star-Ledger, Chase stated,

text: I have no interest in explaining, defending, reinterpreting, or adding to what is there. No one was trying to be audacious, honest to God. We did what we thought we had to do. No one was trying to blow people's minds, or thinking, "Wow, this'll piss them off." People get the impression that you're trying to fuck with them and it's not true. You're trying to entertain them. [...] Anybody who wants to watch it, it's all there.[1]

text: Chase also addressed the opinion of some that the open-ended finale was insulting to the show's longtime fans:

text: I saw some items in the press that said, "This was a huge fuck you to the audience." That we were shitting in the audience's face. Why would we want to do that? Why would we entertain people for eight years only to give them the finger? We don't have contempt for the audience. In fact, I think The Sopranos is the only show that actually gave the audience credit for having some intelligence and attention span. We always operated as though people don't need to be spoon-fed every single thing—that their instincts and feelings and humanity will tell them what's going on.[2][28]

text: In an interview conducted by Brett Martin several weeks after the finale's original broadcast, Chase shared his views on the final episode and the reaction to it. On those fans of the show who demanded an unambiguous and definitive ending, Chase remarked,

text: There was so much more to say than could have been conveyed by an image of Tony facedown in a bowl of onion rings with a bullet in his head. Or, on the other side, taking over the New York mob. The way I see it is that Tony Soprano had been people's alter ego. They had gleefully watched him rob, kill, pillage, lie, and cheat. They had cheered him on. And then, all of a sudden, they wanted to see him punished for all that. They wanted "justice." They wanted to see his brains splattered on the wall. I thought that was disgusting, frankly. [...] The pathetic thing—to me—was how much they wanted his blood, after cheering him on for eight years.

text: Chase also made comments about the purported lack of finality in the final episode:

text: This wasn't really about "leaving the door open." There was nothing definite about what happened, but there was a clean trend on view—a definite sense of what Tony and Carmela's future looks like. Whether it happened that night or some other night doesn't matter.

text: On the future of the Soprano children, Chase said,

text: A.J.'s not going to be citizen-soldier or join the Peace Corps or try to help the world; he'll probably be some low-level movie producer. But he's not going to be a killer like his father, is he? Meadow may not be a pediatrician or even a lawyer, but she's not going to be a housewife like her mother. She'll learn to operate in the world in ways Carmela never did. [...] Tiny, little bits of progress—that's how it works.

text: On moments during and after the final scene, Chase referred to a scene from the episode "Stage 5":

text: There are no esoteric clues in there. No Da Vinci Code. Everything that pertains to that episode was in that episode. And it was in the episode before that and the one before that and seasons before this one and so on. There had been indications of what the end is like. Remember when Gerry Torciano was killed? Silvio was not aware that the gun had been fired until after Gerry was on his way down to the floor. That's the way things happen: It's already going on by the time you even notice it. [...] I'm not saying anything. And I'm not trying to be coy. It's just that I think that to explain it would diminish it.

text: In a December 2008 radio interview with Richard Belzer, Chase also mentioned the scenes from "Stage 5" and "Soprano Home Movies" in relation to the final scene.[29]

text: At the 2008 TCA Awards, held on July 22, Chase commented,

text: I wasn't going to do this, but somebody said it would be a good idea if we said something about that ending. I really wasn't going to go into it, but I'll just say this...when I was going to Stanford University's graduate film school and was 23, I went to see Planet of the Apes with my wife. When it was over, I said, "Wow...so they had a Statue of Liberty, too."[30]

text: In a November 2008 interview with Entertainment Weekly's Steve Daly, Chase stated,

text: "There's more than one way of looking at the ending. That's all I'll say."[31]

text: Chase revisited the final scene in an April 2015 interview with DGA Quarterly[32] and "suggested that fans, experts, and scholars have been over-thinking the ending to the show."[33]

text: “The ceiling I was going for at that point, the biggest feeling I was going for, honestly, was don’t stop believing. It was very simple and much more on the nose than people think. That’s what I wanted people to believe. That life ends and death comes, but don’t stop believing.

text: There are attachments we make in life, even though it’s all going to come to an end, that are worth so much, and we’re so lucky to have been able to experience them. Life is short.

text: Either it ends here for Tony or some other time. But in spite of that, it’s really worth it. So don’t stop believing.”

text: In response to reports that Chase has offered a definitive answer to the question of whether Tony Soprano lived or died, at the show's conclusion,[34][35] Chase has issued denials indicating such reports were incorrect and reiterated the stance he has consistently taken on the subject, and publications have printed retractions.[36][37]

text: Reception[edit]

text: Ratings[edit]

text: According to Nielsen ratings, an average of 11.9 million viewers watched "Made in America" on its United States premiere date Sunday June 10, 2007. This was a 49% increase from the previous episode and the show's best ratings for both parts of the sixth season. It was also the show's largest audience since the season five premiere.[38][39]

text: Response[edit]

text: Initial[edit]

text: "Made in America" received mainly favorable to semi-favorable initial reviews from critics, while early fan reception was mixed to negative, described by one critic as "a mixture of admiration and anger". During the weeks following the episode's original broadcast, "Made in America" and its closing scene in particular became the subject of much discussion and analysis. Several new interpretations and explanations of the ending were presented in magazines and on blogs, which led many critics and fans to reevaluate the ending.[2][15][19][28][40]

text: Marisa Carroll of PopMatters awarded "Made in America" a score of 8 out of 10 and particularly praised the final scene as one of the best of the series.[41] Mark Farinella of The Sun Chronicle called the episode "[a] perfect ending to a perfect TV series."[21] Owen Gleiberman of Entertainment Weekly called "Made in America" "the perfect ending" and wrote about the final scene, "On shock of that cut to black, the marvelous way it got you to roll the scene over, again and again, in your mind's eye. [sic] Rather than bringing the series to a close, that blackout made The Sopranos live forever."[42] Tim Goodman of the San Francisco Chronicle characterized the finale as "[a]n ending befitting genius of Sopranos" and wrote that "Chase managed, with this ending, to be true to reality [...] while also steering clear of trite TV conventions."[43] Frazier Moore of the Associated Press called the episode "brilliant" and wrote that "Chase was true to himself."[44] Kim Reed of Television Without Pity gave "Made in America" the highest score of A+ and praised it for staying true to the show.[45] Alan Sepinwall of The Star-Ledger called the finale "satisfying" and wrote that the episode "fit[s] perfectly with everything Chase has done on this show before."[46] Chicago Tribune critic Maureen Ryan's first review was mixed; she criticized the final scene for not providing any closure. Ryan later wrote: "Chase got me totally wound up, then ripped me away from that world. I was really mad at first [...] I still think what Chase did was, all due respect, kind of jerky. But minutes after the finale ended, I started laughing."[47][48]

text: Retrospective[edit]

text: Retrospective reviews of "Made in America" have been highly positive; the episode has been included on several lists of the best series finales of all time. Alan Sepinwall of The Star-Ledger wrote, in an essay analyzing the finale one year after its original broadcast, that he felt the episode was "brilliant."[40] In 2009, Arlo J. Wiley of Blogcritics wrote: "by focusing on that last ambiguous parting shot from creator David Chase, we run the risk of forgetting just how beautifully structured and executed an hour of television 'Made in America' is" and ranked it as the eighth-best series finale ever.[49] Also in 2009, Stacey Wilson of Film.com named "Made in America" one of the 10 best series finales of all time and wrote: "Crude, rude and no time for emotional B.S., this finale was a delicious end to a show that reveled in the ugliness of humanity."[50] TV Guide included "Made in America" in their "TV's Best Finales Ever" feature, writing: "What's there to say about this finale that hasn't already been said? The much-anticipated closer had everyone waiting to see if Tony was finally going to go from whacker to whackee. Instead, they got Journey, a greasy plate of onion rings and a black screen. But, the fact that we're still talking about it proves—for better or worse—that the episode did its job."[51]

text: In 2011, the finale was ranked #2 on the TV Guide Network special, TV's Most Unforgettable Finales.[52]

text: Awards[edit]

text: In 2007, "Made in America" won an Emmy Award in the category of Outstanding Writing for a Drama Series at the 59th Primetime Emmy Awards. It was the only category the episode was nominated in. This is the third and final time series creator/executive producer David Chase has won the award for his writing of the series.[53] In 2008, Chase was nominated for a Directors Guild of America Award in the category of Drama Series (Night) but lost to fellow Sopranos director Alan Taylor, who won for directing the pilot episode of Mad Men, a series created by former Sopranos writer Matthew Weiner.[54][55] Also in 2008, Editor Sidney Wolinsky won an American Cinema Editors Eddie Award in the category of Best Edited One-Hour Series for Non-Commercial Television.[56]


document_title: Grand Canyon National Park

question_text: when did the grand canyon became a national monument

text: Grand Canyon National Park

text: History[edit]

text: "Grand Canyon" was officially designated a national park on February 26, 1919,[5] though the landmark had been well known to Americans for over thirty years prior.[6] In 1903, President Theodore Roosevelt visited the site and said: "The Grand Canyon fills me with awe. It is beyond comparison—beyond description; absolutely unparalleled through-out the wide world... Let this great wonder of nature remain as it now is. Do nothing to mar its grandeur, sublimity and loveliness. You cannot improve on it. But what you can do is to keep it for your children, your children's children, and all who come after you, as the one great sight which every American should see."[7]

text: Despite Roosevelt's enthusiasm and strong interest in preserving land for public use, the Grand Canyon was not immediately designated as a national park. The first bill to establish Grand Canyon National Park was introduced in 1882 by then-Senator Benjamin Harrison, which would have established Grand Canyon as the second national park in the United States after Yellowstone. Harrison unsuccessfully reintroduced his bill in 1883 and 1886; after his election to the presidency, he established the Grand Canyon Forest Reserve in 1893. Theodore Roosevelt created the Grand Canyon Game Preserve by proclamation on 28 November 1906,[8] and the Grand Canyon National Monument in 1908.[9] Further Senate bills to establish the site as a national park were introduced and defeated in 1910 and 1911, before the Grand Canyon National Park Act was finally signed by President Woodrow Wilson in 1919. The National Park Service, established in 1916, assumed administration of the park.

text: The creation of the park was an early success of the conservation movement. Its national park status may have helped thwart proposals to dam the Colorado River within its boundaries. (Later, the Glen Canyon Dam would be built upriver.) In 1975, the former Marble Canyon National Monument, which followed the Colorado River northeast from the Grand Canyon to Lee's Ferry, was made part of Grand Canyon National Park. In 1979, UNESCO declared the park a World Heritage Site.

text: In 2010, Grand Canyon National Park was honored with its own coin under the America the Beautiful Quarters program.[10]

text: Geography[edit]

text: The Grand Canyon, including its extensive system of tributary canyons, is valued for its combination of size, depth, and exposed layers of colorful rocks dating back to Precambrian times. The canyon itself was created by the incision of the Colorado River and its tributaries after the Colorado Plateau was uplifted, causing the Colorado River system to develop along its present path.

text: The primary public areas of the park are the North and South Rims of the Grand Canyon itself. The rest of the park is extremely rugged and remote, although many places are accessible by pack trail and backcountry roads. Only the Navajo Bridge near Page connects the rims by road in Arizona; this journey can take around five hours by car. Otherwise, the two rims of the Canyon are connected via the Mike O'Callaghan–Pat Tillman Memorial Bridge and the Hoover Dam.[11]

text: The park headquarters are at Grand Canyon Village, not far from the south entrance to the park, near one of the most popular viewpoints.

text: North Rim[edit]

text: The North Rim is a smaller, more remote area with less tourist activity. It is accessed by Arizona State Route 67.[12]

text: South Rim[edit]

text: The South Rim is more accessible than the North Rim;[13] most visitors to the park come to the South Rim, arriving on Arizona State Route 64. The highway enters the park through the South Entrance, near Tusayan, Arizona, and heads eastward, leaving the park through the East Entrance.[13] Interstate 40 provides access to the area from the south. From the north, U.S. Route 89 connects Utah, Colorado, and the North Rim to the South Rim.[14] Overall, some 30 miles of the South Rim are accessible by road.[citation needed]

text: Services[edit]

text: Grand Canyon Village is located at the north end of U.S. Route 180, coming from Flagstaff. It is a full-service community, including lodging, fuel, food, souvenirs, a hospital, churches, and access to trails and guided walks and talks.[11]

text: Lodging[edit]

text: Several lodging facilities are available along the South Rim. Hotels and other lodging include: El Tovar, Bright Angel Lodge, Kachina Lodge, Thunderbird Lodge, and Maswik Lodge, all of which are located in the village area, and Phantom Ranch, located on the canyon floor. There is also an RV Park named Trailer Village. All of these facilities are managed by Xanterra Parks & Resorts, while the Yavapai Lodge (also in the village area) is managed by Delaware North.[15]

text: On the North rim there is the historic Grand Canyon Lodge[15] managed by Forever Resorts and a campground near the lodge, managed by the National Park staff.[16]

text: Activities[edit]

text: South Rim[edit]

text: A variety of activities at the South Rim cater to park visitors. The South Rim Drive (35 miles (56 km) is a driving tour split into two segments. The western drive to Hermit's Point is 8 miles (13 km) with several overlooks along the way, including Mohave Point, Hopi Point, and the Powell Memorial.[11] From March to December, access to Hermit's Rest is restricted to the free shuttle provided by the Park Service. The eastern portion to Desert View is 25 miles (40 km), and is open to private vehicles year round.

text: Walking tours include the Rim Trail, which runs west from the Pipe Creek viewpoint for about 8 miles (13 km) of paved road, followed by 7 miles (11 km) unpaved to Hermit's Rest. Hikes can begin almost anywhere along this trail, and a shuttle can return hikers to their point of origin. Mather Point, the first view most people reach when entering from the South Entrance, is a popular place to begin.

text: Private canyon flyovers are provided by helicopters and small airplanes out of Las Vegas, Phoenix, and Grand Canyon National Park Airport. Due to a crash in the 1990s, scenic flights are no longer allowed to fly within 1,500 feet (460 m) of the rim within the Grand Canyon National Park.[17] Flights within the canyon are still available outside of park boundaries.[18]

text: North Rim[edit]

text: On the North Rim there are few roads, however, there are some notable vehicle accessible lookout points including Point Imperial, Roosevelt Point, and Cape Royal. Mule rides are also available that go to a variety of places including several thousand feet down into the canyon.

text: Many visitors to the North Rim choose to make use of the variety of hiking trails including the Widforss Trail, Uncle Jim's Trail, the Transept Trail, and the North Kaibab Trail, the latter of which can be followed all the way down to the Colorado River, and to across to the South Kaibab Trail and the Bright Angel Trail, which continue up to the south rim of the Grand Canyon.

text: The Toroweap Overlook is located in the western part of the park on the North Rim. Access is via unpaved roads off Route 389 west of Fredonia, Arizona. The roads lead through Grand Canyon-Parashant National Monument and to the overlook.

text: Development[edit]

text: The US government had halted development of a 1.6 million acres area including the National Park from 1966 to 2009, during the Bennett Freeze, because of an ownership dispute between Hopi and Navajo.[19]

text: Grand Canyon Association[edit]

text: The Grand Canyon Association (GCA) is the National Park Service's official nonprofit partner. It raises private funds to benefit Grand Canyon National Park by operating retail shops and visitor centers within the park, and providing educational opportunities about the natural and cultural history of the region.

text: Gallery[edit]

text:
1938 poster of the park

Little Colorado River

Colorado River from the South Rim

A rockfall from the North Rim

From the South Rim in winter

America The Beautiful Quarter