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The chemical elements can be broadly divided into metals, metalloids, and nonmetals according to their shared physical and chemical properties. All elemental metals have a shiny appearance (at least when freshly polished); are good conductors of heat and electricity; form alloys with other metallic elements; and have at least one basic oxide. Metalloids are metallic-looking, often brittle solids that are either semiconductors or exist in semiconducting forms, and have amphoteric or weakly acidic oxides. Typical elemental nonmetals have a dull, coloured or colourless appearance; are often brittle when solid; are poor conductors of heat and electricity; and have acidic oxides. Most or some elements in each category share a range of other properties; a few elements have properties that are either anomalous given their category, or otherwise extraordinary.
Elemental metals appear lustrous (beneath any patina); form compounds (alloys) when combined with other elements; tend to lose or share electrons when they react with other substances; and each forms at least one predominantly basic oxide.
Some metals appear coloured (Cu, Cs, Au), have low densities (e.g. Be, Al) or very high melting points (e.g. W, Nb), are liquids at or near room temperature (e.g. Hg, Ga), are brittle (e.g. Os, Bi), not easily machined (e.g. Ti, Re), or are noble (hard to oxidise, e.g. Au, Pt), or have nonmetallic structures (Mn and Ga are structurally analogous to, respectively, white P and I).
Metalloids are metallic-looking often brittle solids; tend to share electrons when they react with other substances; have weakly acidic or amphoteric oxides; and are usually found naturally in combined states.
Most are semiconductors, and moderate thermal conductors, and have structures that are more open than those of most metals.
Some metalloids (As, Sb) conduct electricity like metals.
The metalloids, as the smallest major category of elements, are not subdivided further.
Nonmetals
25 ml of bromine, a dark red-brown liquid at room temperature
Nonmetallic elements have open structures; tend to gain or share electrons when they react with other substances; and do not form distinctly basic oxides.
Most are gases at room temperature; have relatively low densities; are poor electrical and thermal conductors; have relatively high ionisation energies and electronegativities; form acidic oxides; and are found naturally in uncombined states in large amounts.
Some nonmetals (black P, S, and Se) are brittle solids at room temperature (although each of these also have malleable, pliable or ductile allotropes).
From left to right in the periodic table, the nonmetals can be divided into the reactive nonmetals and the noble gases. The reactive nonmetals near the metalloids show some incipient metallic character, such as the metallic appearance of graphite, black phosphorus, selenium and iodine. The noble gases are almost completely inert.
Comparison of properties
Overview
Number of metalloid properties that resemble metals or nonmetals
The characteristic properties of elemental metals and nonmetals are quite distinct, as shown in the table below. Metalloids, straddling the metal-nonmetal border, are mostly distinct from either, but in a few properties resemble one or the other, as shown in the shading of the metalloid column below and summarized in the small table at the top of this section.
Authors differ in where they divide metals from nonmetals and in whether they recognize an intermediate metalloid category. Some authors count metalloids as nonmetals with weakly nonmetallic properties.[n 1] Others count some of the metalloids as post-transition metals.[n 2]
There were exceptions... in the periodic table, anomalies too—some of them profound. Why, for example, was manganese such a bad conductor of electricity, when the elements on either side of it were reasonably good conductors? Why was strong magnetism confined to the iron metals? And yet these exceptions, I was somehow convinced, reflected special additional mechanisms at work...
The common notions that "alkali metal ions (group 1A) always have a +1 charge"[136] and that "transition elements do not form anions"[137] are textbook errors. The synthesis of a crystalline salt of the sodium anion Na− was reported in 1974. Since then further compounds ("alkalides") containing anions of all other alkali metals except Li and Fr, as well as that of Ba, have been prepared. In 1943, Sommer reported the preparation of the yellow transparent compound CsAu. This was subsequently shown to consist of caesium cations (Cs+) and auride anions (Au−) although it was some years before this conclusion was accepted. Several other aurides (KAu, RbAu) have since been synthesized, as well as the red transparent compound Cs2Pt which was found to contain Cs+ and Pt2− ions.[138]
Well-behaved metals have crystal structures featuring unit cells with up to four atoms. Manganese has a complex crystal structure with a 58-atom unit cell, effectively four different atomic radii, and four different coordination numbers (10, 11, 12 and 16). It has been described as resembling "a quaternary intermetallic compound with four Mn atom types bonding as if they were different elements."[139] The half-filled 3d shell of manganese appears to be the cause of the complexity. This confers a large magnetic moment on each atom. Below 727°C, a unit cell of 58 spatially diverse atoms represents the energetically lowest way of achieving a zero net magnetic moment.[140] The crystal structure of manganese makes it a hard and brittle metal, with low electrical and thermal conductivity. At higher temperatures "greater lattice vibrations nullify magnetic effects"[139] and manganese adopts less-complex structures.[141]
The only elements strongly attracted to magnets are iron, cobalt, and nickel at room temperature, gadolinium just below, and terbium, dysprosium, holmium, erbium, and thulium at ultra-cold temperatures (below −54°C, −185°C, −254°C, −254°C, and −241°C respectively).[142]
The only element encountered with an oxidation state of +9 is iridium, in the [IrO4]+ cation. Other than this, the highest known oxidation state is +8, in Ru, Xe, Os, Ir, and Hs.[143]
The malleability of gold is extraordinary: a fist-sized lump can be hammered and separated into one million paperback-sized sheets, each 10 nm thick,[citation needed] 1600 times thinner than regular kitchen aluminium foil (0.016 mm thick).[citation needed]
Bricks and bowling balls will float on the surface of mercury thanks to it having a density 13.5 times that of water. Equally, a solid mercury bowling ball would weigh around 50 pounds and, if it could be kept cold enough, would float on the surface of liquid gold.[citation needed]
The only metal having an ionisation energy higher than some nonmetals (sulfur and selenium) is mercury.[citation needed]
Mercury and its compounds have a reputation for toxicity but on a scale of 1 to 10, dimethylmercury ((CH3)2Hg) (abbr. DMM), a volatile colourless liquid, has been described as a 15. It is so dangerous that scientists have been encouraged to use less-toxic mercury compounds wherever possible. In 1997, Karen Wetterhahn, a professor of chemistry specialising in toxic metal exposure, died of mercury poisoning ten months after a few drops of DMM landed on her "protective" latex gloves. Although Wetterhahn had been following the then-published procedures for handling this compound, it passed through her gloves and skin within seconds. It is now known that DMM is exceptionally permeable to (ordinary) gloves, skin, and tissues. And its toxicity is such that less than one-tenth of a ml applied to the skin will be seriously toxic.[144]
The expression, to "go down like a lead balloon" is anchored in the common view of lead as a dense, heavy metal—being nearly as dense as mercury. However, it is possible to construct a balloon made of lead foil, filled with a helium and air mixture, which will float and be buoyant enough to carry a small load.[citation needed]
Bismuth has the longest half-life of any naturally occurring element; its only primordial isotope, bismuth-209, was found in 2003 to be slightly radioactive, decaying via alpha decay with a half-life more than a billion times the estimated age of the universe. Prior to this discovery, bismuth-209 was thought to be the heaviest naturally occurring stable isotope;[145] this distinction now belongs to lead-208.
The only element with a naturally occurring isotope capable of undergoing nuclear fission is uranium.[146] The capacity of uranium-235 to undergo fission was first suggested (and ignored) in 1934, and subsequently discovered in 1938.[n 28]
It is normally true that metals reduce their electrical conductivity when heated. Plutonium increases its electrical conductivity when heated in the temperature range of around –175 to +125°C.[149] There is evidence that this behavior, and similar with some of the other transuranic elements is due to more complex relativistic and spin interactions that are not captured by simple model of electrical conductivity.[150]
These elements are record holders within the field of superacid chemistry. For seven decades, fluorosulfonic acid HSO3F and trifluoromethanesulfonic acid CF3SO3H were the strongest known acids that could be isolated as single compounds. Both are about a thousand times more acidic than pure sulfuric acid. In 2004, a boron compound broke this record by a thousand fold with the synthesis of carborane acid H(CHB11Cl11). Another metalloid, antimony, features in the strongest known acid, a mixture 10 billion times stronger than carborane acid. This is fluoroantimonic acid H2F[SbF6], a mixture of antimony pentafluoride SbF5 and hydrofluoric acid HF.[citation needed]
The thermal conductivity of silicon is better than that of most metals.[citation needed]
A sponge-like porous form of silicon (p-Si) is typically prepared by the electrochemical etching of silicon wafers in a hydrofluoric acid solution.[152] Flakes of p-Si sometimes appear red;[153] it has a band gap of 1.97–2.1 eV.[154] The many tiny pores in porous silicon give it an enormous internal surface area, up to 1,000 m2/cm3.[155] When exposed to an oxidant,[156] especially a liquid oxidant,[155] the high surface-area to volume ratio of p-Si creates a very efficient burn, accompanied by nano-explosions,[152] and sometimes by ball-lightning-like plasmoids with, for example, a diameter of 0.1–0.8 m, a velocity of up to 0.5m/s and a lifetime of up to 1s.[157] The first ever spectrographic analysis of a ball lightning event (in 2012) revealed the presence of silicon, iron and calcium, these elements also being present in the soil.[158]
Metals are said to be fusible, resulting in some confusion in old chemistry as to whether arsenic was a true metal, or a nonmetal, or something in-between. It sublimes rather than melts at standard atmospheric pressure, like the nonmetals carbon and red phosphorus.[citation needed]
A high-energy explosive form of antimony was first produced in 1858. It is prepared by the electrolysis of any of the heavier antimony trihalides (SbCl3, SbBr3, SbI3) in a hydrochloric acid solution at low temperature. It comprises amorphous antimony with some occluded antimony trihalide (7–20% in the case of the trichloride). When scratched, struck, powdered or heated quickly to 200°C, it "flares up, emits sparks and is converted explosively into the lower-energy, crystalline grey antimony".[159]
Water (H2O), a well-known oxide of hydrogen, is a spectacular anomaly.[160] Extrapolating from the heavier hydrogen chalcogenides, namely hydrogen sulfide H2S, hydrogen selenide H2Se, and hydrogen telluride H2Te, water should be "a foul-smelling, poisonous, inflammable gas... condensing to a nasty liquid [at] around –100°C". Instead, due to hydrogen bonding, water is "stable, potable, odorless, benign, and... indispensable to life".[161]
Less well-known of the oxides of hydrogen is the trioxide, H2O3. Berthelot proposed the existence of this oxide in 1880 but his suggestion was soon forgotten as there was no way of testing it using the technology of the time.[162] Hydrogen trioxide was prepared in 1994 by replacing the oxygen used in the industrial process for making hydrogen peroxide, with ozone. The yield is about 40 per cent, at –78°C; above around –40°C it decomposes into water and oxygen.[163] Derivatives of hydrogen trioxide, such as F3C–O–O–O–CF3 ("bis(trifluoromethyl) trioxide") are known; these are metastable at room temperature.[164]Mendeleev went a step further, in 1895, and proposed the existence of hydrogen tetroxideHO–O–O–OH as a transient intermediate in the decomposition of hydrogen peroxide;[162] this was prepared and characterised in 1974, using a matrix isolation technique.[citation needed]Alkali metalozonide salts of the unknown hydrogen ozonide (HO3) are also known; these have the formula MO3.[164]
At temperatures below 0.3 and 0.8 K respectively, helium-3 and helium-4 each have a negative enthalpy of fusion. This means that, at the appropriate constant pressures, these substances freeze with the addition of heat.[citation needed]
Until 1999 helium was thought to be too small to form a cage clathrate—a compound in which a guest atom or molecule is encapsulated in a cage formed by a host molecule—at atmospheric pressure. In that year the synthesis of microgram quantities of He@C20H20 represented the first such helium clathrate and (what was described as) the world's smallest helium balloon.[165]
Graphite is the most electrically conductive nonmetal, better than some metals.[citation needed]
Diamond is the best natural conductor of heat; it even feels cold to the touch. Its thermal conductivity (2,200W/m•K) is five times greater than the most conductive metal (Ag at 429); 300 times higher than the least conductive metal (Pu at 6.74); and nearly 4,000 times that of water (0.58) and 100,000 times that of air (0.0224). This high thermal conductivity is used by jewelers and gemologists to separate diamonds from imitations.[citation needed]
Graphene aerogel, produced in 2012 by freeze-drying a solution of carbon nanotubes and graphite oxide sheets and chemically removing oxygen, is seven times lighter than air, and ten per cent lighter than helium. It is the lightest solid known (0.16mg/cm3), conductive and elastic.[166]
The least stable and most reactive form of phosphorus is the whiteallotrope. It is a hazardous, highly flammable and toxic substance, spontaneously igniting in air and producing phosphoric acid residue. It is therefore normally stored under water. White phosphorus is also the most common, industrially important, and easily reproducible allotrope, and for these reasons is regarded as the standard state of phosphorus. The most stable form is the black allotrope, which is a metallic looking, brittle and relatively non-reactive semiconductor (unlike the white allotrope, which has a white or yellowish appearance, is pliable, highly reactive and a semiconductor). When assessing periodicity in the physical properties of the elements it needs to be borne in mind that the quoted properties of phosphorus tend to be those of its least stable form rather than, as is the case with all other elements, the most stable form.[citation needed]
The mildest of the halogens, iodine is the active ingredient in tincture of iodine, a disinfectant. This can be found in household medicine cabinets or emergency survival kits. Tincture of iodine will rapidly dissolve gold,[167] a task ordinarily requiring the use of aqua regia (a highly corrosive mixture of nitric and hydrochloric acids).[citation needed]
Eby et al.[4] discuss the weak chemical behaviour of the elements close to the metal-nonmetal borderline.
Booth and Bloom[5] say "A period represents a stepwise change from elements strongly metallic to weakly metallic to weakly nonmetallic to strongly nonmetallic, and then, at the end, to an abrupt cessation of almost all chemical properties...".
Cox[6] notes "nonmetallic elements close to the metallic borderline (Si, Ge, As, Sb, Se, Te) show less tendency to anionic behaviour and are sometimes called metalloids."
↑ See, for example, Huheey, Keiter & Keiter[7] who classify Ge and Sb as post-transition metals.
↑ At standard pressure and temperature, for the elements in their most thermodynamically stable forms, unless otherwise noted
↑ Copernicium is reported to be the only metal known to be a gas at room temperature.[20]
↑ Whether polonium is ductile or brittle is unclear. It is predicted to be ductile based on its calculated elastic constants.[25] It has a simple cubic crystalline structure. Such a structure has few slip systems and "leads to very low ductility and hence low fracture resistance".[26]
↑ Carbon as exfoliated (expanded) graphite,[28] and as metre-long carbon nanotube wire;[29] phosphorus as white phosphorus (soft as wax, pliable and can be cut with a knife, at room temperature);[30] sulfur as plastic sulfur;[31] and selenium as selenium wires.[32]
↑ For polycrystalline forms of the elements unless otherwise noted. Determining Poisson's ratio accurately is a difficult proposition and there could be considerable uncertainty in some reported values.[33]
↑ Beryllium has the lowest known value (0.0476) among elemental metals; indium and thallium each have the highest known value (0.46). Around one third show a value ≥ 0.33.[34]
↑ The Goldhammer-Herzfeld criterion is a ratio that compares the force holding an individual atom's valence electrons in place with the forces, acting on the same electrons, arising from interactions between the atoms in the solid or liquid element. When the interatomic forces are greater than or equal to the atomic force, valence electron itinerancy is indicated. Metallic behaviour is then predicted.[58] Otherwise nonmetallic behaviour is anticipated. The Goldhammer-Herzfeld criterion is based on classical arguments.[59] It nevertheless offers a relatively simple first order rationalization for the occurrence of metallic character among the elements.[60]
↑ Metals have electrical conductivity values of from 6.9 × 103 S•cm−1 for manganese to 6.3 × 105 for silver.[63]
↑ Metalloids have electrical conductivity values of from 1.5 × 10−6 S•cm−1 for boron to 3.9 × 104 for arsenic.[65] If selenium is included as a metalloid the applicable conductivity range would start from ~10−9 to 10−12 S•cm−1.[66][67][68]
↑ Nonmetals have electrical conductivity values of from ~10−18 S•cm−1 for the elemental gases to 3 × 104 in graphite.[69]
↑ Mott and Davis[71] note however that 'liquid europium has a negative temperature coefficient of resistance' i.e. that conductivity increases with rising temperature
↑ Chedd[94] defines metalloids as having electronegativity values of 1.8 to 2.2 (Allred-Rochow scale). He included boron, silicon, germanium, arsenic, antimony, tellurium, polonium and astatine in this category. In reviewing Chedd's work, Adler[95] described this choice as arbitrary, given other elements have electronegativities in this range, including copper, silver, phosphorus, mercury, and bismuth. He went on to suggest defining a metalloid simply as, 'a semiconductor or semimetal' and 'to have included the interesting materials bismuth and selenium in the book'.
↑ Phosphorus is known to form a carbide in thin films.
↑ Sulfates of osmium have not been characterized with any great degree of certainty.[107]
↑ Common metalloids: Boron is reported to be capable of forming an oxysulfate (BO)2SO4,[108] a bisulfate B(HSO4)3[109] and a sulfate B2(SO4)3.[110] The existence of a sulfate has been disputed.[111] In light of the existence of silicon phosphate, a silicon sulfate might also exist.[112] Germanium forms an unstable sulfate Ge(SO4)2 (d 200 °C).[113] Arsenic forms oxide sulfates As2O(SO4)2 (= As2O3.2SO3)[114] and As2(SO4)3 (= As2O3.3SO3).[115] Antimony forms a sulfate Sb2(SO4)3 and an oxysulfate (SbO)2SO4.[116] Tellurium forms an oxide sulfate Te2O3(SO)4.[117]Less common: Polonium forms a sulfate Po(SO4)2.[118] It has been suggested that the astatine cation forms a weak complex with sulfate ions in acidic solutions.[119]
↑ Hydrogen forms hydrogen sulfate H2SO4. Carbon forms (a blue) graphite hydrogen sulfate C+ 24HSO– 4•2.4H2SO4.[120] Nitrogen forms nitrosyl hydrogen sulfate (NO)HSO4 and nitronium (or nitryl) hydrogen sulfate (NO2)HSO4.[121] There are indications of a basic sulfate of selenium SeO2.SO3 or SeO(SO4).[122] Iodine forms a polymeric yellow sulfate (IO)2SO4.[123]
↑ Based on a table of the elemental composition of the biosphere, and lithosphere (crust, atmosphere, and seawater) in Georgievskii,[131] and the masses of the crust and hydrosphere give in Lide and Frederikse.[132] The mass of the biosphere is negligible, having a mass of about one billionth that of the lithosphere.[citation needed] "The oceans constitute about 98 percent of the hydrosphere, and thus the average composition of the hydrosphere is, for all practical purposes, that of seawater."[133]
↑ Hydrogen gas is produced by some bacteria and algae and is a natural component of flatus. It can be found in the Earth's atmosphere at a concentration of 1 part per million by volume.
↑ Fluorine can be found in its elemental form, as an occlusion in the mineral antozonite[135]
↑ In 1934, a team led by Enrico Fermi postulated that transuranic elements may have been produced as a result of bombarding uranium with neutrons, a finding which was widely accepted for a few years. In the same year Ida Noddack, a German scientist and subsequently a three-time Nobel prize nominee, criticised this assumption, writing "It is conceivable that the nucleus breaks up into several large fragments, which would of course be isotopes of known elements but would not be neighbors of the irradiated element."[147][emphasis added] In this, Noddak defied the understanding of the time without offering experimental proof or theoretical basis, but nevertheless presaged what would be known a few years later as nuclear fission. Her paper was generally ignored as, in 1925, she and two colleagues claimed to have discovered element 43, then proposed to be called masurium (later discovered in 1936 by Perrier and Segrè, and named technetium). Had Ida Noddack's paper been accepted it is likely that Germany would have had an atomic bomb and, 'the history of the world would have been [very] different.'[148]
↑ Jauncey 1948, p.500: 'Nonmetals mostly have negative temperature coefficients. For instance, carbon... [has a] resistance [that] decreases with a rise in temperature. However, recent experiments on very pure graphite, which is a form of carbon, have shown that pure carbon in this form behaves similarly to metals in regard to its resistance.'
Barium is a chemical element; it has symbol Ba and atomic number 56. It is the fifth element in group 2 and is a soft, silvery alkaline earth metal. Because of its high chemical reactivity, barium is never found in nature as a free element.
The chalcogens are the chemical elements in group 16 of the periodic table. This group is also known as the oxygen family. Group 16 consists of the elements oxygen (O), sulfur (S), selenium (Se), tellurium (Te), and the radioactive elements polonium (Po) and livermorium (Lv). Often, oxygen is treated separately from the other chalcogens, sometimes even excluded from the scope of the term "chalcogen" altogether, due to its very different chemical behavior from sulfur, selenium, tellurium, and polonium. The word "chalcogen" is derived from a combination of the Greek word khalkos (χαλκός) principally meaning copper, and the Latinized Greek word genēs, meaning born or produced.
A metal is a material that, when polished or fractured, shows a lustrous appearance, and conducts electricity and heat relatively well. These properties are all associated with having electrons available at the Fermi level, as against nonmetallic materials which do not. Metals are typically ductile and malleable.
The periodic table, also known as the periodic table of the elements, is an ordered arrangement of the chemical elements into rows ("periods") and columns ("groups"). It is an icon of chemistry and is widely used in physics and other sciences. It is a depiction of the periodic law, which states that when the elements are arranged in order of their atomic numbers an approximate recurrence of their properties is evident. The table is divided into four roughly rectangular areas called blocks. Elements in the same group tend to show similar chemical characteristics.
A metalloid is a chemical element which has a preponderance of properties in between, or that are a mixture of, those of metals and nonmetals. The word metalloid comes from the Latin metallum ("metal") and the Greek oeides. There is no standard definition of a metalloid and no complete agreement on which elements are metalloids. Despite the lack of specificity, the term remains in use in the literature.
In the context of the periodic table a nonmetal is a chemical element that mostly lacks distinctive metallic properties. They range from colorless gases like hydrogen to shiny crystals like iodine. Physically, they are usually lighter than elements that form metals and are often poor conductors of heat and electricity. Chemically, nonmetals have relatively high electronegativity or usually attract electrons in a chemical bond with another element, and their oxides tend to be acidic.
A period 3 element is one of the chemical elements in the third row of the periodic table of the chemical elements. The periodic table is laid out in rows to illustrate recurring (periodic) trends in the chemical behavior of the elements as their atomic number increases: a new row is begun when chemical behavior begins to repeat, meaning that elements with similar behavior fall into the same vertical columns. The third period contains eight elements: sodium, magnesium, aluminium, silicon, phosphorus, sulfur, chlorine and argon. The first two, sodium and magnesium, are members of the s-block of the periodic table, while the others are members of the p-block. All of the period 3 elements occur in nature and have at least one stable isotope.
Sulfide (also sulphide in British English) is an inorganic anion of sulfur with the chemical formula S2− or a compound containing one or more S2− ions. Solutions of sulfide salts are corrosive. Sulfide also refers to large families of inorganic and organic compounds, e.g. lead sulfide and dimethyl sulfide. Hydrogen sulfide (H2S) and bisulfide (HS−) are the conjugate acids of sulfide.
In chemistry and physics, valence electrons are electrons in the outermost shell of an atom, and that can participate in the formation of a chemical bond if the outermost shell is not closed. In a single covalent bond, a shared pair forms with both atoms in the bond each contributing one valence electron.
In chemistry, catenation is the bonding of atoms of the same element into a series, called a chain. A chain or a ring may be open if its ends are not bonded to each other, or closed if they are bonded in a ring. The words to catenate and catenation reflect the Latin root catena, "chain".
This is a list of 194 sources that list elements classified as metalloids. The sources are listed in chronological order. Lists of metalloids differ since there is no rigorous widely accepted definition of metalloid. Individual lists share common ground, with variations occurring at the margins. The elements most often regarded as metalloids are boron, silicon, germanium, arsenic, antimony and tellurium. Other sources may subtract from this list, add a varying number of other elements, or both.
The origin and usage of the term metalloid is convoluted. Its origin lies in attempts, dating from antiquity, to describe metals and to distinguish between typical and less typical forms. It was first applied to metals that floated on water, and then more popularly to nonmetals. Only recently, since the mid-20th century, has it been widely used to refer to elements with intermediate or borderline properties between metals and nonmetals.
The dividing line between metals and nonmetals can be found, in varying configurations, on some representations of the periodic table of the elements. Elements to the lower left of the line generally display increasing metallic behaviour; elements to the upper right display increasing nonmetallic behaviour. When presented as a regular stair-step, elements with the highest critical temperature for their groups lie just below the line.
Fluorine forms a great variety of chemical compounds, within which it always adopts an oxidation state of −1. With other atoms, fluorine forms either polar covalent bonds or ionic bonds. Most frequently, covalent bonds involving fluorine atoms are single bonds, although at least two examples of a higher order bond exist. Fluoride may act as a bridging ligand between two metals in some complex molecules. Molecules containing fluorine may also exhibit hydrogen bonding. Fluorine's chemistry includes inorganic compounds formed with hydrogen, metals, nonmetals, and even noble gases; as well as a diverse set of organic compounds. For many elements the highest known oxidation state can be achieved in a fluoride. For some elements this is achieved exclusively in a fluoride, for others exclusively in an oxide; and for still others the highest oxidation states of oxides and fluorides are always equal.
The metallic elements in the periodic table located between the transition metals to their left and the chemically weak nonmetallic metalloids to their right have received many names in the literature, such as post-transition metals, poor metals, other metals, p-block metals, basic metals, and chemically weak metals. The most common name, post-transition metals, is generally used in this article.
Nonmetals show more variability in their properties than do metals. Metalloids are included here since they behave predominately as chemically weak nonmetals.
Nonmetallic material, or in nontechnical terms a nonmetal, refers to materials which are not metals. Depending upon context it is used in slightly different ways. In everyday life it would be a generic term for those materials such as plastics, wood or ceramics which are not typical metals such as the iron alloys used in bridges. In some areas of chemistry, particularly the periodic table, it is used for just those chemical elements which are not metallic at standard temperature and pressure conditions. It is also sometimes used to describe broad classes of dopant atoms in materials. In general usage in science, it refers to materials which do not have electrons that can readily move around, more technically there are no available states at the Fermi energy, the equilibrium energy of electrons. For historical reasons there is a very different definition of metals in astronomy, with just hydrogen and helium as nonmetals. The term may also be used as a negative of the materials of interest such as in metallurgy or metalworking.
References
Addison WE 1964, The allotropy of the elements, Oldbourne Press, London
Adler D 1969, 'Half-way elements: The technology of metalloids', book review, Technology Review, vol. 72, no. 1, Oct/Nov, pp.18–19
Benedict M, Alvarez LW, Bliss LA, English SG, Kinzell AB, Morrison P, English FH, Starr C & Williams WJ 1946, 'Technological control of atomic energy activities', "Bulletin of the Atomic Scientists", vol. 2, no. 11, pp.18–29
Askeland DR, Fulay PP & Wright JW 2011, The science and engineering of materials, 6th ed., Cengage Learning, Stamford, CT, ISBN0-495-66802-8
Atkins P, Overton T, Rourke J, Weller M & Armstrong F 2006, Shriver & Atkins' inorganic chemistry, 4th ed., Oxford University Press, Oxford, ISBN0-7167-4878-9
Austen K 2012, 'A factory for elements that barely exist', NewScientist, 21 Apr, p.12, ISSN 1032-1233
Bagnall KW 1966, The chemistry of selenium, tellurium and polonium, Elsevier, Amsterdam
Bailar JC, Moeller T, Kleinberg J, Guss CO, Castellion ME & Metz C 1989, Chemistry, 3rd ed., Harcourt Brace Jovanovich, San Diego, ISBN0-15-506456-8
Bassett LG, Bunce SC, Carter AE, Clark HM & Hollinger HB 1966, Principles of chemistry, Prentice-Hall, Englewood Cliffs, NJ
Batsanov SS & Batsanov AS 2012, Introduction to structural chemistry, Springer Science+Business Media, Dordrecht, ISBN978-94-007-4770-8
Berei K & Vasáros L 1985, 'Astatine compounds', in Kugler & Keller
Betke, Ulf; Wickleder, Mathias S. (2011-01-05). "Sulfates of the Refractory Metals: Crystal Structure and Thermal Behavior of Nb2O2(SO4)3, MoO2(SO4), WO(SO4)2, and Two Modifications of Re2O5(SO4)2". Inorganic Chemistry. 50 (3). American Chemical Society (ACS): 858–872. doi:10.1021/ic101455z. ISSN0020-1669. PMID21207946.
Beveridge TJ, Hughes MN, Lee H, Leung KT, Poole RK, Savvaidis I, Silver S & Trevors JT 1997, 'Metal–microbe interactions: Contemporary approaches', in RK Poole (ed.), Advances in microbial physiology, vol. 38, Academic Press, San Diego, pp.177–243, ISBN0-12-027738-7
Bogoroditskii NP & Pasynkov VV 1967, Radio and electronic materials, Iliffe Books, London
Booth VH & Bloom ML 1972, Physical science: a study of matter and energy, Macmillan, New York
Brassington, M. P.; Lambson, W. A.; Miller, A. J.; Saunders, G. A.; Yogurtçu, Y. K. (1980). "The second- and third-order elastic constants of amorphous arsenic". Philosophical Magazine B. 42 (1). Informa UK Limited: 127–148. Bibcode:1980PMagB..42..127B. doi:10.1080/01418638008225644. ISSN1364-2812.
Brasted RC 1974, 'Oxygen group elements and their compounds', in The new Encyclopædia Britannica, vol. 13, Encyclopædia Britannica, Chicago, pp.809–824
Brescia F, Arents J, Meislich H & Turk A 1975, Fundamentals of chemistry, 3rd ed., Academic Press, New York, p.453, ISBN978-0-12-132372-1
Brinkley SR 1945, Introductory general chemistry, 3rd ed., Macmillan, New York
Brown TL, LeMay HE, Bursten BE, Murphy CJ & Woodward P 2009, Chemistry: The Central Science, 11th ed., Pearson Education, New Jersey, ISBN978-0-13-235-848-4
Burakowski T & Wierzchoń T 1999, Surface engineering of metals: Principles, equipment, technologies, CRC Press, Boca Raton, Fla, ISBN0-8493-8225-4
Bychkov VL 2012, 'Unsolved Mystery of Ball Lightning', in Atomic Processes in Basic and Applied Physics, V Shevelko & H Tawara (eds), Springer Science & Business Media, Heidelberg, pp.3–24, ISBN978-3-642-25568-7
Carapella SC 1968a, 'Arsenic' in CA Hampel (ed.), The encyclopedia of the chemical elements, Reinhold, New York, pp.29–32
Cerkovnik, Janez; Plesničar, Božo (2013-06-28). "Recent Advances in the Chemistry of Hydrogen Trioxide (HOOOH)". Chemical Reviews. 113 (10). American Chemical Society (ACS): 7930–7951. doi:10.1021/cr300512s. ISSN0009-2665. PMID23808683.
Chang R 1994, Chemistry, 5th (international) ed., McGraw-Hill, New York
Chang R 2002, Chemistry, 7th ed., McGraw Hill, Boston
Chedd G 1969, Half-way elements: The technology of metalloids, Doubleday, New York
Clementi, E.; Raimondi, D. L.; Reinhardt, W. P. (1967-08-15). "Atomic Screening Constants from SCF Functions. II. Atoms with 37 to 86 Electrons". The Journal of Chemical Physics. 47 (4). AIP Publishing: 1300–1307. Bibcode:1967JChPh..47.1300C. doi:10.1063/1.1712084. ISSN0021-9606.
Cordes EH & Scaheffer R 1973, Chemistry, Harper & Row, New York
Cotton SA 1994, 'Scandium, yttrium & the lanthanides: Inorganic & coordination chemistry', in RB King (ed.), Encyclopedia of inorganic chemistry, 2nd ed., vol. 7, John Wiley & Sons, New York, pp.3595–3616, ISBN978-0-470-86078-6
Donohoe J 1982, The Structures of the Elements, Robert E. Krieger, Malabar, Florida, ISBN0-89874-230-7
Douglade, J.; Mercier, R. (1982-03-15). "Structure cristalline et covalence des liaisons dans le sulfate d'arsenic(III), As2(SO4)3". Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry. 38 (3). International Union of Crystallography (IUCr): 720–723. doi:10.1107/s056774088200394x. ISSN0567-7408.
Dunstan S 1968, Principles of chemistry, D. Van Nostrand Company, London
Du Plessis M 2007, 'A Gravimetric Technique to Determine the Crystallite Size Distribution in High Porosity Nanoporous Silicon, in JA Martino, MA Pavanello & C Claeys (eds), Microelectronics Technology and Devices–SBMICRO 2007, vol. 9, no. 1, The Electrochemical Society, New Jersey, pp.133–142, ISBN978-1-56677-565-6
Eby GS, Waugh CL, Welch HE & Buckingham BH 1943, The physical sciences, Ginn and Company, Boston
Edwards, Peter P.; Sienko, M. J. (1983). "On the occurrence of metallic character in the periodic table of the elements". Journal of Chemical Education. 60 (9). American Chemical Society (ACS): 691–696. Bibcode:1983JChEd..60..691E. doi:10.1021/ed060p691. ISSN0021-9584.
Edwards PP 1999, 'Chemically engineering the metallic, insulating and superconducting state of matter' in KR Seddon & M Zaworotko (eds), Crystal engineering: The design and application of functional solids, Kluwer Academic, Dordrecht, pp.409–431
Edwards PP 2000, 'What, why and when is a metal?', in N Hall (ed.), The new chemistry, Cambridge University, Cambridge, pp.85–114
Fraden, J. H. (1951). "Amorphous antimony. A lecture demonstration in allotropy". Journal of Chemical Education. 28 (1): 34-35. doi:10.1021/ed028p34. ISSN0021-9584.
Furuseth, Sigrid; Selte, Kari; Hope, Håkon; Kjekshus, Arne; Klewe, Bernt; Powell, D. L. (1974). "Iodine Oxides. Part V. The Crystal Structure of (IO)2SO4". Acta Chemica Scandinavica. 28a: 71–76. doi:10.3891/acta.chem.scand.28a-0071. ISSN0904-213X.
Georgievskii VI 1982, 'Biochemical regions. Mineral composition of feeds', in VI Georgievskii, BN Annenkov & VT Samokhin (eds), Mineral nutrition of animals: Studies in the agricultural and food sciences, Butterworths, London, pp.57–68, ISBN0-408-10770-7
Gillespie RJ & Robinson EA 1959, 'The sulphuric acid solvent system', in HJ Emeléus & AG Sharpe (eds), Advances in inorganic chemistry and radiochemistry, vol. 1, Academic Press, New York, pp.386–424
Glazov VM, Chizhevskaya SN & Glagoleva NN 1969, Liquid semiconductors, Plenum, New York
Glinka N 1965, General chemistry, trans. D Sobolev, Gordon & Breach, New York
Gösele U & Lehmann V 1994, 'Porous Silicon Quantum Sponge Structures: Formation Mechanism, Preparation Methods and Some Properties', in Feng ZC & Tsu R (eds), Porous Silicon, World Scientific, Singapore, pp.17–40, ISBN981-02-1634-3
Greaves, G. N.; Greer, A. L.; Lakes, R. S.; Rouxel, T. (2011). "Poisson's ratio and modern materials". Nature Materials. 10 (11): 823–837. doi:10.1038/nmat3134. ISSN1476-1122. PMID22020006.
Greenwood NN & Earnshaw A 2002, Chemistry of the elements, 2nd ed., Butterworth-Heinemann, ISBN0-7506-3365-4
Gschneidner, Karl A. (1964). "Physical Properties and Interrelationships of Metallic and Semimetallic Elements". Solid State Physics. Vol.16. Elsevier. p.275-426. doi:10.1016/s0081-1947(08)60518-4. ISBN978-0-12-607716-2.
Habashi F 2003, Metals from ores: an introduction to extractive metallurgy, Métallurgie Extractive Québec, Sainte Foy, Québec, ISBN2-922686-04-3
Manson SS & Halford GR 2006, Fatigue and Durability of Structural Materials, ASM International, Materials Park, OH, ISBN0-87170-825-6
Hampel CA & Hawley GG 1976, Glossary of chemical terms, Van Nostrand Reinhold, New York
Hem JD 1985, Study and interpretation of the chemical characteristics of natural water, paper 2254, 3rd ed., US Geological Society, Alexandria, Virginia
Herzfeld, K. F. (1927-05-01). "On Atomic Properties which make an Element a Metal". Physical Review. 29 (5): 701–705. doi:10.1103/PhysRev.29.701. ISSN0031-899X.
Heslop RB & Robinson PL 1963, Inorganic chemistry: A guide to advanced study, Elsevier, Amsterdam
Hiller LA & Herber RH 1960, Principles of chemistry, McGraw-Hill, New York
Holtzclaw HF, Robinson WR & Odom JD 1991, General chemistry, 9th ed., DC Heath, Lexington, ISBN0-669-24429-5
Hopcroft, Matthew A.; Nix, William D.; Kenny, Thomas W. (2010). "What is the Young's Modulus of Silicon?". Journal of Microelectromechanical Systems. 19 (2): 229–238. doi:10.1109/JMEMS.2009.2039697. ISSN1057-7157.
Huheey JE, Keiter EA & Keiter RL 1993, Principles of Structure & Reactivity, 4th ed., HarperCollins College Publishers, ISBN0-06-042995-X
Hultgren HH 1966, 'Metalloids', in GL Clark & GG Hawley (eds), The encyclopedia of inorganic chemistry, 2nd ed., Reinhold Publishing, New York
Hunt A 2000, The complete A-Z chemistry handbook, 2nd ed., Hodder & Stoughton, London
Iler RK 1979, The chemistry of silica: solubility, polymerization, colloid and surface properties, and biochemistry, John Wiley, New York, ISBN978-0-471-02404-0
Jauncey GEM 1948, Modern physics: A second course in college physics, D. Von Nostrand, New York
Jenkins GM & Kawamura K 1976, Polymeric carbons—carbon fibre, glass and char, Cambridge University Press, Cambridge
Keenan CW, Kleinfelter DC & Wood JH 1980, General college chemistry, 6th ed., Harper & Row, San Francisco, ISBN0-06-043615-8
Keogh DW 2005, 'Actinides: Inorganic & coordination chemistry', in RB King (ed.), Encyclopedia of inorganic chemistry, 2nd ed., vol. 1, John Wiley & Sons, New York, pp.2–32, ISBN978-0-470-86078-6
Klein CA & Cardinale GF 1992, 'Young's modulus and Poisson's ratio of CVD diamond', in A Feldman & S Holly, SPIE Proceedings, vol. 1759, Diamond Optics V, pp.178‒192, doi:10.1117/12.130771
Kneen WR, Rogers MJW & Simpson P 1972, Chemistry: Facts, patterns, and principles, Addison-Wesley, London
Kovalev, D.; Timoshenko, V. Yu.; Künzner, N.; Gross, E.; Koch, F. (2001-07-19). "Strong Explosive Interaction of Hydrogenated Porous Silicon with Oxygen at Cryogenic Temperatures". Physical Review Letters. 87 (6): 068301. doi:10.1103/PhysRevLett.87.068301. ISSN0031-9007. PMID11497868.
Kozyrev PT 1959, 'Deoxidized selenium and the dependence of its electrical conductivity on pressure. II', Physics of the solid state, translation of the journal Solid State Physics (Fizika tverdogo tela) of the Academy of Sciences of the USSR, vol. 1, pp.102–110
Kugler HK & Keller C (eds) 1985, Gmelin Handbook of Inorganic and Organometallic chemistry, 8th ed., 'At, Astatine', system no. 8a, Springer-Verlag, Berlin, ISBN3-540-93516-9
Lagrenaudie J 1953, 'Semiconductive properties of boron' (in French), Journal de chimie physique, vol. 50, nos. 11–12, Nov-Dec, pp.629–633
Lazaruk, S. K.; Dolbik, A. V.; Labunov, V. A.; Borisenko, V. E. (2007). "Combustion and explosion of nanostructured silicon in microsystem devices". Semiconductors. 41 (9): 1113–1116. doi:10.1134/S1063782607090175. ISSN1063-7826.
Legut, Dominik; Friák, Martin; Šob, Mojmír (2010-06-22). "Phase stability, elasticity, and theoretical strength of polonium from first principles". Physical Review B. 81 (21): 214118. doi:10.1103/PhysRevB.81.214118. ISSN1098-0121.
Leith MM 1966, Velocity of sound in solid iodine, MSc thesis, University of British Columbia. Leith comments that, '...as iodine is anisotropic in many of its physical properties most attention was paid to two amorphous samples which were thought to give representative average values of the properties of iodine' (p. iii).
Lide DR & Frederikse HPR (eds) 1998, CRC Handbook of chemistry and physics, 79th ed., CRC Press, Boca Raton, Florida, ISBN0-849-30479-2
Lidin RA 1996, Inorganic substances handbook, Begell House, New York, ISBN1-56700-065-7
Andersen, A. Lindegaard; Dahle, Birgit (1966-01-01). "Fracture Phenomena in Amorphous Selenium". Journal of Applied Physics. 37 (1): 262–266. doi:10.1063/1.1707823. ISSN0021-8979.
Mann, Joseph B.; Meek, Terry L.; Allen, Leland C. (2000-03-01). "Configuration Energies of the Main Group Elements". Journal of the American Chemical Society. 122 (12): 2780–2783. doi:10.1021/ja992866e. ISSN0002-7863.
Marlowe MO 1970, Elastic properties of three grades of fine grained graphite to 2000°C, NASA CR‒66933, National Aeronautics and Space Administration, Scientific and Technical Information Facility, College Park, Maryland
Martienssen W & Warlimont H (eds) 2005, Springer Handbook of Condensed Matter and Materials Data, Springer, Heidelberg, ISBN3-540-30437-1
Matula, R. A. (1979-10-01). "Electrical resistivity of copper, gold, palladium, and silver". Journal of Physical and Chemical Reference Data. 8 (4): 1147–1298. doi:10.1063/1.555614. ISSN0047-2689.
McQuarrie DA & Rock PA 1987, General chemistry, 3rd ed., WH Freeman, New York
Mendeléeff DI 1897, The Principles of Chemistry, vol. 2, 5th ed., trans. G Kamensky, AJ Greenaway (ed.), Longmans, Green & Co., London
Mercier, R.; Douglade, J. (1982-06-15). "Structure cristalline d'un oxysulfate d'arsenic(III) As2O(SO4)2 (ou As2O3.2SO3)". Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry. 38 (6): 1731–1735. doi:10.1107/S0567740882007055.
Metcalfe HC, Williams JE & Castka JF 1966, Modern chemistry, 3rd ed., Holt, Rinehart and Winston, New York
Moss TS 1952, Photoconductivity in the Elements, London, Butterworths
Mott NF & Davis EA 2012, 'Electronic Processes in Non-Crystalline Materials', 2nd ed., Oxford University Press, Oxford, ISBN978-0-19-964533-6
Nakao, Yukimichi (1992). "Dissolution of noble metals in halogen–halide–polar organic solvent systems". Journal of the Chemical Society, Chemical Communications (5): 426–427. doi:10.1039/C39920000426. ISSN0022-4936.
Nemodruk AA & Karalova ZK 1969, Analytical chemistry of boron, R Kondor trans., Ann Arbor Humphrey Science, Ann Arbor, Michigan
New Scientist 1975, 'Chemistry on the islands of stability', 11 Sep, p.574, ISSN 1032-1233
Perkins D 1998, Mineralogy, Prentice Hall Books, Upper Saddle River, New Jersey, ISBN0-02-394501-X
Pottenger FM & Bowes EE 1976, Fundamentals of chemistry, Scott, Foresman and Co., Glenview, Illinois
Qin, Jiaqian; Nishiyama, Norimasa; Ohfuji, Hiroaki; Shinmei, Toru; Lei, Li; He, Duanwei; Irifune, Tetsuo (2012). "Polycrystalline γ-boron: As hard as polycrystalline cubic boron nitride". Scripta Materialia. 67 (3): 257–260. arXiv:1203.1748. doi:10.1016/j.scriptamat.2012.04.032.
Rao, C.N.R.; Ganguly, P. (1986). "A new criterion for the metallicity of elements". Solid State Communications. 57 (1): 5–6. doi:10.1016/0038-1098(86)90659-9.
Raub CJ & Griffith WP 1980, 'Osmium and sulphur', in Gmelin handbook of inorganic chemistry, 8th ed., 'Os, Osmium: Supplement', K Swars (ed.), system no. 66, Springer-Verlag, Berlin, pp.166–170, ISBN3-540-93420-0
Ravindran, P.; Fast, Lars; Korzhavyi, P. A.; Johansson, B.; Wills, J.; Eriksson, O. (1998-11-01). "Density functional theory for calculation of elastic properties of orthorhombic crystals: Application to TiSi2". Journal of Applied Physics. 84 (9): 4891–4904. doi:10.1063/1.368733. ISSN0021-8979.
Reynolds WN 1969, Physical properties of graphite, Elsevier, Amsterdam
Rochow EG 1966, The metalloids, DC Heath and Company, Boston
Rock PA & Gerhold GA 1974, Chemistry: Principles and applications, WB Saunders, Philadelphia
Russell JB 1981, General chemistry, McGraw-Hill, Auckland
Sacks O 2001, Uncle Tungsten: Memories of a chemical boyhood, Alfred A Knopf, New York, ISBN0-375-40448-1
Sanderson RT 1960, Chemical periodicity, Reinhold Publishing, New York
Sanderson RT 1967, Inorganic chemistry, Reinhold, New York
Sanderson K 2012, 'Stinky rocks hide Earth's only haven for natural fluorine', Nature News, July, doi:10.1038/nature.2012.10992
Schaefer JC 1968, 'Boron' in CA Hampel (ed.), The encyclopedia of the chemical elements, Reinhold, New York, pp.73–81
Sidgwick NV 1950, The chemical elements and their compounds, vol. 1, Clarendon, Oxford
Sidorov, T. A. (1960). "The connection between structural oxides and their tendency to glass formation". Glass and Ceramics. 17 (11): 599–603. doi:10.1007/BF00670116. ISSN0361-7610.
Sisler HH 1973, Electronic structure, properties, and the periodic law, Van Nostrand, New York
Slough W 1972, 'Discussion of session 2b: Crystal structure and bond mechanism of metallic compounds', in O Kubaschewski (ed.), Metallurgical chemistry, proceedings of a symposium held at Brunel University and the National Physical Laboratory on the 14, 15 and 16 July 1971, Her Majesty's Stationery Office [for the] National Physical Laboratory, London
Slyh JA 1955, 'Graphite', in JF Hogerton & RC Grass (eds), Reactor handbook: Materials, US Atomic Energy Commission, McGraw Hill, New York, pp.133‒154
Smith A 1921, General chemistry for colleges, 2nd ed., Century, New York
Sneed MC 1954, General college chemistry, Van Nostrand, New York
Rao, R. V. G. Sundara (1950). "Elastic constants of orthorhombic sulphur". Proceedings of the Indian Academy of Sciences - Section A. 32 (4): 275-278. doi:10.1007/BF03170831. ISSN0370-0089.
Sundara Rao RVG 1954, 'Erratum to: Elastic constants of orthorhombic sulphur', Proceedings of the Indian Academy of Sciences, Section A, vol. 40, no. 3, p.151
Swalin RA 1962, Thermodynamics of solids, John Wiley & Sons, New York
Tilley RJD 2004, Understanding solids: The science of materials, 4th ed., John Wiley, New York
Walker JD, Newman MC & Enache M 2013, Fundamental QSARs for metal ions, CRC Press, Boca Raton, ISBN978-1-4200-8434-4
White, Mary Anne; Cerqueira, Anthony B.; Whitman, Catherine A.; Johnson, Michel B.; Ogitsu, Tadashi (2015-03-16). "Determination of Phase Stability of Elemental Boron". Angewandte Chemie International Edition. 54 (12): 3626–3629. doi:10.1002/anie.201409169. ISSN1433-7851. PMID25619645.
Wickleder, M. S.; Pley, M.; Büchner, O. (2006). "Sulfates of Precious Metals: Fascinating Chemistry of Potential Materials". Zeitschrift für anorganische und allgemeine Chemie. 632 (12–13): 2080. doi:10.1002/zaac.200670009. ISSN0044-2313.
Wickleder MS 2007, 'Chalcogen-oxygen chemistry', in FA Devillanova (ed.), Handbook of chalcogen chemistry: new perspectives in sulfur, selenium and tellurium, RSC, Cambridge, pp.344–377, ISBN978-0-85404-366-8
Wilson JR 1965, 'The structure of liquid metals and alloys', Metallurgical reviews, vol. 10, p.502
Wilson AH 1966, Thermodynamics and statistical mechanics, Cambridge University, Cambridge
Witczak Z, Goncharova VA & Witczak PP 2000, 'Irreversible effect of hydrostatic pressure on the elastic properties of polycrystalline tellurium', in MH Manghnani, WJ Nellis & MF Nicol (eds), Science and technology of high pressure: Proceedings of the International Conference on High Pressure Science and Technology (AIRAPT-17), Honolulu, Hawaii, 25‒30 July 1999, vol. 2, Universities Press, Hyderabad, pp.822‒825, ISBN81-7371-339-1
Witt SF 1991, 'Dimethylmercury', Occupational Safety & Health Administration Hazard Information Bulletin, US Department of Labor, February 15, accessed 8 May 2015
Wittenberg, Layton J.; DeWitt, Robert (1972-05-01). "Volume Contraction During Melting; Emphasis on Lanthanide and Actinide Metals". The Journal of Chemical Physics. 56 (9): 4526–4533. doi:10.1063/1.1677899. ISSN0021-9606.
Young RV & Sessine S (eds) 2000, World of chemistry, Gale Group, Farmington Hills, Michigan
Zhigal'skii GP & Jones BK 2003, Physical properties of thin metal films, Taylor & Francis, London, ISBN0-415-28390-6
Zuckerman & Hagen (eds) 1991, Inorganic reactions and methods, vol, 5: The formation of bonds to group VIB (O, S, Se, Te, Po) elements (part 1), VCH Publishers, Deerfield Beach, Fla, ISBN0-89573-250-5
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