Properties of metals, metalloids and nonmetals - wikipedia Properties of metals, metalloids and nonmetals The periodic table showing : metals in most of the left and centre ; metalloids in a narrow diagonal band ; nonmetals in the right, and hydrogen The chemical elements can be broadly divided into metals, metalloids and nonmetals according to their shared physical and chemical properties. All metals have a shiny appearance ( at least when freshly polished ) ; are good conductors of heat and electricity ; form alloys with other metals ; and have at least one basic oxide. Metalloids are metallic - looking brittle solids that are either semiconductors or exist in semiconducting forms, and have amphoteric or weakly acidic oxides. Typical nonmetals have a dull, coloured or colourless appearance ; are 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. Contents 1 Properties 1.1 Metals 1.2 Metalloids 1.3 Nonmetals 2 Comparison of properties 2.1 Overview 2.2 Detailed 3 Anomalous properties 3.1 Metals 3.2 Metalloids 3.3 Nonmetals 4 Notes 5 Citations 6 References Properties Metals Pure ( 99.97 % + ) iron chips, electrolytically refined, accompanied by a high purity ( 99.9999 % = 6N ) 1 cm cube Main article : Metal Metals appear lustrous ( beneath any patina ) ; form mixtures ( alloys ) when combined with other metals ; tend to lose or share electrons when they react with other substances ; and each forms at least one predominantly basic oxide. Most metals are silvery looking, high density, relatively soft and easily deformed solids with good electrical and thermal conductivity, closely packed structures, low ionisation energies and electronegativities, and are found naturally in combined states. Some metals appear coloured ( Cu, Cs, Au ), have low densities ( e.g. Be, Al ) or very high melting points, are liquids at or near room temperature, are brittle ( e.g. Os, Bi ), not easily machined ( e.g. Ti, Re ), or are noble ( hard to oxidise ) or have nonmetallic structures ( Mn and Ga are structurally analogous to, respectively, white P and I ). Metals comprise the large majority of the elements, and can be subdivided into several different categories. From left to right in the periodic table, these categories include the highly reactive alkali metals ; the less reactive alkaline earth metals, lanthanides and radioactive actinides ; the archetypal transition metals, and the physically and chemically weak post-transition metals. Specialized subcategories such as the refractory metals and the noble metals also exist. Metalloids Tellurium, described by Dmitri Mendeleev as forming a transition between metals and nonmetals Main article : Metalloid Metalloids are metallic looking 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 Main article : Nonmetal Nonmetals have open structures ( unless solidified from gaseous or liquid forms ) ; 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 ( C, 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 subdivided into the polyatomic nonmetals which, being nearest to the metalloids, show some incipient metallic character ; the diatomic nonmetals, which are essentially nonmetallic ; and the monatomic noble gases, which are almost completely inert. Comparison of properties Overview Number of metalloid properties that resemble metals or nonmetals ( or that are reasonably distinct ) Resemble metals Relatively distinctive Resemble nonmetals Properties compared : ( 36 ) 7 ( 19 % ) 25 ( 68 % ) 5 ( 13 % ) Physical ( 21 ) 5 ( 24 % ) 14 ( 67 % ) 2 ( 10 % ) Presentation & structure ( 10 ) 2 6 2 ( 20 % ) Electron - related ( 6 ) 1 5 Thermodynamics ( 5 ) 2 3 Chemical ( 16 ) 2 ( 13 % ) 11 ( 69 % ) 3 ( 19 % ) Elemental chemistry ( 6 ) 3 3 ( 50 % ) Combined form chemistry ( 6 ) 2 4 Environmental chemistry ( 4 ) 4 The characteristic properties of 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. Others count some of the metalloids as post-transition metals. Detailed Physical and chemical properties Metals Metalloids Nonmetals Presentation and structure Colour nearly all are shiny and grey - white Cu, Cs, Au : shiny and golden shiny and grey - white most are colourless or dull red, yellow, green, or intermediate shades C, P, Se, I : shiny and grey - white Reflectivity intermediate to typically high intermediate zero or low ( mostly ) to intermediate Form almost all solid Rb, Cs, Fr, Ga, Hg : liquid at / near stp all solid most are gases C, P, S, Se, I : solid ; Br : liquid Density generally high, with some exceptions such as the alkali metals lower than nearby metals but higher than nearby nonmetals often low Deformability ( as a solid ) most are ductile and malleable some are brittle ( Cr, Mn, Ga, Ru, W, Os, Bi ) brittle brittle, when solid some ( C, P, S, Se ) have non-brittle forms Poisson 's ratio low to high low to intermediate low to intermediate Crystalline structure at freezing point most are hexagonal or cubic Ga, U, Np : orthorhombic ; In, Sn, Pa : tetragonal ; Sm, Hg, Bi : rhombohedral ; Pu : monoclinic B, As, Sb : rhombohedral Si, Ge : cubic Te : hexagonal H, He, C, N, Se : hexagonal O, F, Ne, P, Ar, Kr, Xe, Rn : cubic S, Cl, Br, I : orthorhombic Packing & coordination number close - packed crystal structures high coordination numbers relatively open crystal structures medium coordination numbers open structures low coordination numbers Atomic radius ( calculated ) intermediate to very large 112 -- 298 pm, average 187 small to intermediate : B, Si, Ge, As, Sb, Te 87 -- 123 pm, average 115.5 pm very small to intermediate 31 -- 120 pm, average 76.4 pm Allotropes around half form allotropes one ( Sn ) has a metalloid - like allotrope ( grey Sn, which forms below 13.2 ° C ) all or nearly all form allotropes some ( e.g. red B, yellow As ) are more nonmetallic in nature some form allotropes some ( e.g. graphitic C, black P, grey Se ) are more metalloidal or metallic in nature Electron - related Periodic table block s, p, d, f p s, p Outer s and p electrons few in number ( 1 -- 3 ) except 0 ( Pd ) ; 4 ( Sn, Pb, Fl ) ; 5 ( Bi ) ; 6 ( Po ) medium number ( 3 -- 7 ) high number ( 4 -- 8 ) except 1 ( H ) ; 2 ( He ) Electron bands : ( valence, conduction ) nearly all have substantial band overlap Bi : has slight band overlap ( semimetal ) most have narrow band gap ( semiconductors ) As, Sb are semimetals most have wide band gap ( insulators ) C ( graphite ) : a semimetal P ( black ), Se, I : semiconductors Electron behaviour `` free '' electrons ( facilitating electrical and thermal conductivity ) valence electrons less freely delocalized ; considerable covalent bonding present have Goldhammer - Herzfeld criterion ratios straddling unity no, few, or directionally confined `` free '' electrons ( generally hampering electrical and thermal conductivity ) Electrical conductivity good to high intermediate to good poor to good... as a liquid falls gradually as temperature rises most behave like metals increases as temperature rises Thermodynamics Thermal conductivity medium to high mostly intermediate ; Si is high almost negligible to very high Temperature coefficient of resistance nearly all positive ( Pu is negative ) negative ( B, Si, Ge, Te ) or positive ( As, Sb ) nearly all negative ( C, as graphite, is positive in the direction of its planes ) Melting point very high and solid at room temperature ( except mercury ) very high and solid at room temperature mostly low and gas at room temperature Melting behaviour volume generally expands some contract, unlike ( most ) metals volume generally expands Enthalpy of fusion low to high intermediate to very high very low to low ( except C : very high ) Elemental chemistry Overall behaviour metallic nonmetallic nonmetallic Ion formation tend to form cations some tendency to form anions in water solution chemistry dominated by formation and reactions of oxyanions tend to form anions Bonds seldom form covalent compounds form salts as well as covalent compounds form many covalent compounds Oxidation number nearly always positive positive or negative positive or negative Ionization energy relatively low intermediate high Electronegativity usually low close to 2, i.e., 1.9 -- 2.2 high Combined form chemistry With metals form alloys can form alloys form ionic or interstitial compounds With carbon carbides and organometallic compounds same as metals carbon - nonmetal ( e.g. CO, CS ) or organic ( e.g. CH, C H O ) compounds With hydrogen ( hydrides ) ionic, with alkali, alkaline earth metals metallic, with transition metals covalent, with post-transition metals covalent, volatile hydrides covalent, gaseous or liquid hydrides With oxygen ( oxides ) nearly all solid ( Mn O is a liquid ) very few glass formers lower oxides : ionic and basic higher oxides : more covalent, acidic solid glass formers ( B, Si, Ge, As, Sb, Te ) polymeric in structure ; tend to be amphoteric or weakly acidic solid, liquid or gaseous few glass formers ( P, S, Se ) covalent, acidic With sulfur ( sulfates ) do form most form some form With halogens ( halides, esp. chlorides ) ( see also ) typically ionic, involatile generally insoluble in organic solvents mostly water - soluble ( not hydrolysed ) more covalent, volatile, and susceptible to hydrolysis and organic solvents with higher halogens and weaker metals covalent, volatile usually dissolve in organic solvents partly or completely hydrolysed some reversibly hydrolysed covalent, volatile usually dissolve in organic solvents generally completely or extensively hydrolyzed not always susceptible to hydrolysis if parent nonmetal at maximum covalency for period e.g. CF, SF ( then nil reaction ) Environmental chemistry Molar composition of Earth 's ecosphere about 14 %, mostly Al, Na, Ng, Ca, Fe, K about 17 %, mostly Si about 69 %, mostly O, H Primary form on Earth most occur in combined states, as carbonates, silicates, phosphates, oxides, sulfides, or halides some ( e.g. Au, Cu, Ag, Pt ) occur in free or uncombined states all occur in combined states, as borates, silicates, sulfides, or tellurides elemental C, N, O, S, noble gases are plentiful H, F, Se occur primarily in compounds P, Cl, Br, I occur only in compounds, as phosphates, oxides, selenides or halides Required by mammals large amounts needed : Na, Mg, K, Ca trace amounts needed of some others trace amounts needed : B, Si, As large amounts needed : H, C, N, O, P, S, Cl trace amounts needed : Se, Br, I, possibly F only noble gases not needed Composition of the human body, by weight about 1.5 % Ca traces of most others through U trace amounts of B, Si, Ge, As, Sb, Te about 97 % O, C, H, N, P others detectable except noble gases Anomalous properties 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... `` '' Oliver Sacks Uncle Tungsten ( 2001, p. 204 ) Within each category, elements can be found with one or two properties very different from the expected norm, or that are otherwise notable. Metals Sodium, potassium, rubidium, caesium, barium, platinum, gold The common notions that `` alkali metal ions ( group 1A ) always have a + 1 charge '' and that `` transition elements do not form anions '' 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 Cs Pt which was found to contain Cs and Pt ions. Manganese 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. '' 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. 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 '' and manganese adopts less complex structures. Iron, cobalt, nickel, gadolinium, terbium, dysprosium, holmium, erbium, thulium 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 ). Iridium The only element encountered with an oxidation state of + 9 is iridium, in the ( IrO ) cation. Other than this, the highest known oxidation state is + 8, in Ru, Xe, Os, Ir, and Hs. Gold The malleability of gold is extraordinary : a fist sized lump can be hammered and separated into one million paper back sized sheets, each 10 nm thick, 1600 times thinner than regular kitchen aluminium foil ( 0.016 mm thick ). Mercury 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. The only metal having an ionisation energy higher than some nonmetals ( sulfur and selenium ) is mercury. Mercury and its compounds have a reputation for toxicity but on a scale of 1 to 10, dimethylmercury ( ( CH ) Hg ) ( 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. Lead 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. Bismuth 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 ; this distinction now belongs to lead - 208. Uranium The only element with a naturally occurring isotope capable of undergoing nuclear fission is uranium. The capacity of uranium - 235 to undergo fission was first suggested ( and ignored ) in 1934, and subsequently discovered in 1938. Plutonium It is a commonly held belief 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. Metalloids Boron Boron is the only element with a partially disordered structure in its most thermodynamically stable crystalline form. Boron, antimony These elements are record holders within the field of superacid chemistry. For seven decades, fluorosulfonic acid HSO F and trifluoromethanesulfonic acid CF SO H 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 ( CHB Cl ). Another metalloid, antimony, features in the strongest known acid, a mixture 10 billion times stronger than carborane acid. This is fluoroantimonic acid H F ( SbF ), a mixture of antimony pentafluoride SbF and hydrofluoric acid HF. Silicon The thermal conductivity of silicon is better than that of most metals. A sponge - like porous form of silicon ( p - Si ) is typically prepared by the electrochemical etching of silicon wafers in a hydrofluoric acid solution. Flakes of p - Si sometimes appear red ; it has a band gap of 1.97 -- 2.1 eV. The many tiny pores in porous silicon give it an enormous internal surface area, up to 1,000 m / cm. When exposed to an oxidant, especially a liquid oxidant, the high surface - area to volume ratio of p - Si creates a very efficient burn, accompanied by nano - explosions, and sometimes by ball - lightning - like plasmoids with, for example, a diameter of 0.1 -- 0.8 m, a velocity of up to 0.5 m / s and a lifetime of up to 1s. 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. Arsenic 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. Antimony A high - energy explosive form of antimony was first obtained in 1858. It is prepared by the electrolysis of any of the heavier antimony trihalides ( SbCl, SbBr, SbI ) 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. '' Nonmetals Hydrogen Water ( H O ), a well known oxide of hydrogen, is a spectacular anomaly. Extrapolating from the heavier hydrogen chalcogenides, namely hydrogen sulfide H S, hydrogen selenide H Se, and hydrogen telluride H Te, 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 ''. Less well known of the oxides of hydrogen is the trioxide, H O. 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. 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. Derivatives of hydrogen trioxide, such as F C -- O -- O -- O -- CF ( `` bis ( trifluoromethyl ) trioxide '' ) are known ; these are metastable at room temperature. Mendeleev went a step further, in 1895, and proposed the existence of hydrogen tetroxide HO -- O -- O -- OH as a transient intermediate in the decomposition of hydrogen peroxide ; this was prepared and characterised in 1974, using a matrix isolation technique. Alkali metal ozonide salts of the unknown hydrogen ozonide ( HO ) are also known ; these have the formula MO. Helium 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. 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@C H represented the first such helium clathrate and ( what was described as ) the world 's smallest helium balloon. Carbon Graphite is the most electrically conductive nonmetal, better than some metals. Diamond is the best natural conductor of heat ; it even feels cold to the touch. Its thermal conductivity ( 2,200 W / 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. 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 ( 0.16 mg / cm ), conductive and elastic. Phosphorus The least stable and most reactive form of phosphorus is the white allotrope. 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. Iodine 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, a task ordinarily requiring the use of aqua regia ( a highly corrosive mixture of nitric and hydrochloric acids ). Notes Jump up ^ For example : Brinkley writes that boron has weakly nonmetallic properties. Glinka describes silicon as a weak nonmetal. Eby et al. discuss the weak chemical behaviour of the elements close to the metal - nonmetal borderline. Booth and Bloom 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 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. '' Jump up ^ See, for example, Huheey, Keiter & Keiter who classify Ge and Sb as post-transition metals. Jump up ^ At standard pressure and temperature, for the elements in their most thermodynamically stable forms, unless otherwise noted Jump up ^ Copernicium is reported to be the only metal known to be a gas at room temperature. Jump up ^ Whether polonium is ductile or brittle is unclear. It is predicted to be ductile based on its calculated elastic constants. 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 ''. Jump up ^ Carbon as exfoliated ( expanded ) graphite, and as metre - long carbon nanotube wire ; phosphorus as white phosphorus ( soft as wax, pliable and can be cut with a knife, at room temperature ) ; sulfur as plastic sulfur ; and selenium as selenium wires. Jump up ^ 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. Jump up ^ Beryllium has the lowest known value ( 0.0476 ) amongst elemental metals ; indium and thallium each have the highest known value ( 0.46 ). Around one third show a value ≥ 0.33. Jump up ^ Boron 0.13 ; silicon 0.22 ; germanium 0.278 ; amorphous arsenic 0.27 ; antimony 0.25 ; tellurium ~ 0.2. Jump up ^ Graphitic carbon 0.25 ; ( diamond 0.0718 ) ; black phosphorus 0.30 ; sulfur 0.287 ; amorphous selenium 0.32 ; amorphous iodine ~ 0. Jump up ^ At atmospheric pressure, for elements with known structures Jump up ^ 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. Otherwise nonmetallic behaviour is anticipated. The Goldhammer - Herzfeld criterion is based on classical arguments. It nevertheless offers a relatively simple first order rationalization for the occurrence of metallic character amongst the elements. Jump up ^ Metals have electrical conductivity values of from 6.9 × 10 S cm for manganese to 6.3 × 10 for silver. Jump up ^ Metalloids have electrical conductivity values of from 1.5 × 10 S cm for boron to 3.9 × 10 for arsenic. If selenium is included as a metalloid the applicable conductivity range would start from ~ 10 to 10 S cm. Jump up ^ Nonmetals have electrical conductivity values of from ~ 10 S cm for the elemental gases to 3 × 10 in graphite. Jump up ^ Mott and Davis note however that ' liquid europium has a negative temperature coefficient of resistance ' i.e. that conductivity increases with rising temperature Jump up ^ At or near room temperature Jump up ^ Chedd 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 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 '. Jump up ^ Phosphorus is known to form a carbide in thin films. Jump up ^ See, for example, the sulfates of the transition metals, the lanthanides and the actinides. Jump up ^ Sulfates of osmium have not been characterized with any great degree of certainty. Jump up ^ Common metalloids : Boron is reported to be capable of forming an oxysulfate ( BO ) SO, a bisulfate B ( HSO ) and a sulfate B ( SO ). The existence of a sulfate has been disputed. In light of the existence of silicon phosphate, a silicon sulfate might also exist. Germanium forms an unstable sulfate Ge ( SO ) ( d 200 ° C ). Arsenic forms oxide sulfates As O ( SO ) ( = As O. 2SO ) and As ( SO ) ( = As O. 3SO ). Antimony forms a sulfate Sb ( SO ) and an oxysulfate ( SbO ) SO. Tellurium forms an oxide sulfate Te O ( SO ). Less common : Polonium forms a sulfate Po ( SO ). It has been suggested that the astatine cation forms a weak complex with sulfate ions in acidic solutions. Jump up ^ Hydrogen forms hydrogen sulfate H SO. Carbon forms ( a blue ) graphite hydrogen sulfate C HSO 2.4 H SO. Nitrogen forms nitrosyl hydrogen sulfate ( NO ) HSO and nitronium ( or nitryl ) hydrogen sulfate ( NO ) HSO. There are indications of a basic sulfate of selenium SeO.SO or SeO ( SO ). Iodine forms a polymeric yellow sulfate ( IO ) SO. Jump up ^ layer - lattice types often reversibly so Jump up ^ Based on a table of the elemental composition of the biosphere, and lithosphere ( crust, atmosphere, and seawater ) in Georgievskii, and the masses of the crust and hydrosphere give in Lide and Frederikse. The mass of the biosphere is negligible, having a mass of about one billionth that of the lithosphere. `` 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. '' Jump up ^ 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. Jump up ^ Fluorine can be found in its elemental form, as an occlusion in the mineral antozonite Jump up ^ 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. '' ( 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. ' Citations Jump up ^ Mendeléeff 1897, p. 274 Jump up ^ Brinkley 1945, p. 378 Jump up ^ Glinka 1965, p. 88 Jump up ^ Eby et al. 1943, p. 404 Jump up ^ Booth & Bloom 1972, p. 426 ^ Jump up to : Cox 2004, p. 27 Jump up ^ Huheey, Keiter & Keiter 1993, p. 28 ^ Jump up to : Kneen, Rogers & Simpson, 1972, p. 263. Columns 2 ( metals ) and 4 ( nonmetals ) are sourced from this reference unless otherwise indicated. Jump up ^ Russell & Lee 2005, p. 147 ^ Jump up to : Rochow 1966, p. 4 Jump up ^ Pottenger & Bowes 1976, p. 138 Jump up ^ Askeland, Fulay & Wright 2011, p. 806 Jump up ^ Born & Wolf 1999, p. 746 Jump up ^ Lagrenaudie 1953 Jump up ^ Rochow 1966, pp. 23, 25 Jump up ^ Burakowski & Wierzchoń 1999, p. 336 Jump up ^ Olechna & Knox 1965, pp. A991 ‒ 92 Jump up ^ Stoker 2010, p. 62 Jump up ^ Chang 2002, p. 304. Chang speculates that the melting point of francium would be about 23 ° C. Jump up ^ New Scientist 1975 ; Soverna 2004 ; Eichler, Aksenov & Belozeroz et al. 2007 ; Austen 2012 Jump up ^ Hunt 2000, p. 256 Jump up ^ Sisler 1973, p. 89 Jump up ^ Hérold 2006, pp. 149 -- 150 Jump up ^ Russell & Lee 2005 Jump up ^ Legit, Friák & Šob 2010, p. 214118 - 18 Jump up ^ Manson & Halford 2006, pp. 378, 410 ^ Jump up to : McQuarrie & Rock 1987, p. 85 Jump up ^ Chung 1987 ; Godfrin & Lauter 1995 Jump up ^ Cambridge Enterprise 2013 Jump up ^ Faraday 1853, p. 42 ; Holderness & Berry 1979, p. 255 Jump up ^ Partington 1944, p. 405 Jump up ^ Regnault 1853, p. 208 Jump up ^ Christensen 2012, p. 14 Jump up ^ Gschneidner 1964, pp. 292 ‒ 93. 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In bulk semimetals... the resistivity will increase with temperature... to give a positive temperature coefficient of resistivity... ' Jump up ^ 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. ' Jump up ^ Reynolds 1969, pp. 91 -- 92 ^ Jump up to : Wilson 1966, p. 260 Jump up ^ Wittenberg 1972, p. 4526 Jump up ^ Habashi 2003, p. 73 Jump up ^ Bailar et al. 1989, p. 742 Jump up ^ Hiller & Herber 1960, inside front cover ; p. 225 Jump up ^ Beveridge et al. 1997, p. 185 ^ Jump up to : Young & Sessine 2000, p. 849 Jump up ^ Bailar et al. 1989, p. 417 Jump up ^ Metcalfe, Williams & Castka 1966, p. 72 Jump up ^ Chang 1994, p. 311 Jump up ^ Pauling 1988, p. 183 Jump up ^ Mann et al. 2000, p. 2783 Jump up ^ Chedd 1969, pp. 24 -- 25 Jump up ^ Adler 1969, pp. 18 -- 19 Jump up ^ Hultgren 1966, p. 648 Jump up ^ Bassett et al. 1966, p. 602 Jump up ^ Rochow 1966, p. 34 Jump up ^ Martienssen & Warlimont 2005, p. 257 Jump up ^ Sidorov 1960 Jump up ^ Brasted 1974, p. 814 Jump up ^ Atkins 2006 et al., pp. 8, 122 -- 23 Jump up ^ Rao 2002, p. 22 Jump up ^ Wickleder, Pley & Büchner 2006 ; Betke & Wickleder 2011 Jump up ^ Cotton 1994, p. 3606 Jump up ^ Keogh 2005, p. 16 Jump up ^ Raub & Griffith 1980, p. 167 Jump up ^ Nemodruk & Karalova 1969, p. 48 Jump up ^ Sneed 1954, p. 472 ; Gillespie & Robinson 1959, p. 407 Jump up ^ Zuckerman & Hagen 1991, p. 303 Jump up ^ Sanderson 1967, p. 178 Jump up ^ Iler 1979, p. 190 Jump up ^ Sanderson 1960, p. 162 ; Greenwood & Earnshaw 2002, p. 387 Jump up ^ Mercier & Douglade 1982 Jump up ^ Douglade & Mercier 1982 Jump up ^ Wiberg 2001, p. 764 Jump up ^ Wickleder 2007, p. 350 Jump up ^ Bagnall 1966, pp. 140 − 41 Jump up ^ Berei & Vasáros 1985, pp. 221, 229 Jump up ^ Wiberg 2001, p. 795 Jump up ^ Lidin 1996, pp. 266, 270 ; Brescia et al. 1975, p. 453 Jump up ^ Greenwood & Earnshaw 2002, p. 786 Jump up ^ Furuseth et al. 1974 Jump up ^ Holtzclaw, Robinson & Odom 1991, pp. 706 -- 07 ; Keenan, Kleinfelter & Wood 1980, pp. 693 -- 95 Jump up ^ Kneen, Rogers & Simpson 1972, p. 278 Jump up ^ Heslop & Robinson 1963, p. 417 Jump up ^ Rochow 1966, pp. 28 -- 29 Jump up ^ Bagnall 1966, pp. 108, 120 ; Lidin 1996, passim ^ Jump up to : Smith 1921, p. 295 ; Sidgwick 1950, pp. 605, 608 ; Dunstan 1968, pp. 408, 438 Jump up ^ Dunstan 1968, pp. 312, 408 Jump up ^ Georgievskii 1982, p. 58 Jump up ^ Lide & Frederikse 1998, p. 14 -- 6 Jump up ^ Hem 1985, p. 7 Jump up ^ Perkins 1998, p. 350 Jump up ^ Sanderson 2012 Jump up ^ Brown et al. 2009, p. 137 Jump up ^ Bresica et al. 1975, p. 137 Jump up ^ Jansen 2005 ^ Jump up to : Russell & Lee 2005, p. 246 Jump up ^ Russell & Lee 2005, p. 244 -- 5 Jump up ^ Donohoe 1982, pp. 191 -- 196 ; Russell & Lee 2005, pp. 244 -- 247 Jump up ^ Jackson 2000 Jump up ^ Stoye 2014 Jump up ^ Witt 1991 ; Endicott 1998 Jump up ^ Dumé 2003 Jump up ^ Benedict et al. 1946, p. 19 Jump up ^ Noddack 1934, p. 653 Jump up ^ Sacks 2001, p. 205 : ' This story was told by Glenn Seaborg when he was presenting his recollections at a conference in November 1997. ' Jump up ^ Dalhouse University 2015 ; White et al. 2015 ^ Jump up to : DuPlessis 2007, p. 133 Jump up ^ Gösele & Lehmann 1994, p. 19 Jump up ^ Chen, Lee & Bosman 1994 ^ Jump up to : Kovalev et al. 2001, p. 068301 - 1 Jump up ^ Mikulec, Kirtland & Sailor 2002 Jump up ^ Bychkov 2012, pp. 20 -- 21 ; see also Lazaruk et al. 2007 Jump up ^ Slezak 2014 Jump up ^ Wiberg 2001, p. 758 ; see also Fraden 1951 Jump up ^ Sacks 2001, p. 204 Jump up ^ Sacks 2001, pp. 204 -- 205 ^ Jump up to : Cerkovnik & Plesničar 2013, p. 7930 Jump up ^ Emsley 1994, p. 1910 ^ Jump up to : Wiberg 2001, p. 497 Jump up ^ Cross, Saunders & Prinzbach ; Chemistry Views 2015 Jump up ^ Sun, Xu & Gao 2013 ; Anthony 2013 Jump up ^ Nakao 1992 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 Anita M 1998, ' Focus : Levitating Liquid Boron ', American Physical Society, viewed 14 December 2014 Anthony S 2013, ' Graphene aerogel is seven times lighter than air, can balance on a blade of grass ', ExtremeTech, April 10, accessed 8 February 2015 Appalakondaiah S, Vaitheeswaran G, Lebègue S, Christensen NE & Svane A 2012, ' Effect of van der Waals interactions on the structural and elastic properties of black phosphorus, ' Physical Review B, vol. 86, pp. 035105 ‒ 1 to 9, doi : 10.1103 / PhysRevB. 86.035105 Askeland DR, Fulay PP & Wright JW 2011, The science and engineering of materials, 6th ed., Cengage Learning, Stamford, CT, ISBN 0 - 495 - 66802 - 8 Atkins P, Overton T, Rourke J, Weller M & Armstrong F 2006, Shriver & Atkins ' inorganic chemistry, 4th ed., Oxford University Press, Oxford, ISBN 0 - 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, ISBN 0 - 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, ISBN 978 - 94 - 007 - 4770 - 8 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 Dumé, Belle ( 23 April 2003 ). `` Bismuth breaks half - life record for alpha decay ''. 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250 - 5 Periodic table Periodic table forms Standard 18 - column 18 - column, large cells 32 - column, large cells Alternative Alternatives Chemical Galaxy Janet 's left step table Extended Extension beyond the 7th period Fricke model large cells Pyykkö model Sets of elements By periodic table structure Groups 1 ( Alkali metals ) 2 ( Alkaline earth metals ) 5 6 7 8 9 10 11 12 13 14 15 ( Pnictogens ) 16 ( Chalcogens ) 17 ( Halogens ) 18 ( Noble gases ) Periods 5 6 7 8 + Aufbau Fricke Pyykkö Blocks s - block p - block d - block f - block g - block Aufbau principle By metallicity Metals Alkali metals Alkaline earth metals Lanthanides Actinides Superactinides Transition metals Post-transition metals Metalloids Lists of metalloids by source Dividing line Nonmetals Polyatomic nonmetals Diatomic nonmetals Noble gases Other sets Nutritional elements Platinum - group metals ( PGM ) Rare - earth elements Refractory metals Precious metals Coinage metals Noble metal Heavy metals Native metals Transuranium elements Transactinide elements Major actinides Minor actinides Elements Lists By : Abundance ( in humans ) Atomic properties Nuclear stability Production Symbol Properties Atomic weight Crystal structure Electron affinity Electron configuration Electronegativity Allen Pauling Goldschmidt classification Maximum valence Data pages Abundance Atomic radius Boiling point Critical point Density Elasticity Electrical resistivity Electron affinity Electron configuration Electronegativity Hardness Heat capacity Heat of fusion Heat of vaporization Ionization energy Melting point Oxidation state Speed of sound Thermal conductivity Thermal expansion coefficient Vapor pressure History Element discoveries Mendeleev 's predictions Naming Etymology controversies places scientists in East Asia See also IUPAC nomenclature systematic element name Trivial name Dmitri Mendeleev Book Chemistry Portal Periodic table ( Large cells ) 5 6 7 8 9 10 11 12 13 14 15 16 17 18 He Li Be O Ne Na Mg Al Si Cl Ar Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te Xe 6 Cs Ba La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Hf Ta Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 7 Fr Ra Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og Alkali metal Alkaline earth metal Lanthanide Actinide Transition metal Post - ​ transition metal Metalloid Polyatomic nonmetal Diatomic nonmetal Noble gas Unknown chemical properties Retrieved from `` https://en.wikipedia.org/w/index.php?title=Properties_of_metals,_metalloids_and_nonmetals&oldid=824209112 '' Categories : Metals Metalloids Nonmetals Hidden categories : All articles with unsourced statements Articles with unsourced statements from February 2015 Articles with unsourced statements from April 2015 Articles with unsourced statements from January 2015 Talk Contents About Wikipedia اردو Edit links This page was last edited on 5 February 2018, at 23 : 50. 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Question: are metals mostly solid liquid or gas at room temperature
Answer: solids