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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.

Properties

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Metals

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.

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 (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).

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

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

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

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. Others count some of the metalloids as post-transition metals.

Details

Anomalous properties

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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...

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 Cs₂Pt 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 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 paperback-sized sheets, each 10 nm thick, 1600 times thinner than regular kitchen aluminium foil (0.016 mm thick).

Mercury

1. 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.
2. The only metal having an ionisation energy higher than some nonmetals (sulfur and selenium) is mercury.
3. 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.

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 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. 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.

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 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, a mixture of antimony pentafluoride SbF₅ and hydrofluoric acid HF.

Silicon

1. The thermal conductivity of silicon is better than that of most metals.
2. 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 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".

Nonmetals

Hydrogen

1. Water (H₂O), a well-known oxide of hydrogen, is a spectacular anomaly. 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 around –100 °C". Instead, due to hydrogen bonding, water is "stable, potable, odorless, benign, and... indispensable to life".
2. 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. 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 F₃C–O–O–O–CF₃ ("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 (HO₃) are also known; these have the formula MO₃.

Helium

1. 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.
2. 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.

Carbon

1. Graphite is the most electrically conductive nonmetal, better than some metals.
2. 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.
3. 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

1. 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."
2. See, for example, Huheey, Keiter & Keiter who classify Ge and Sb as post-transition metals.
3. At standard pressure and temperature, for the elements in their most thermodynamically stable forms, unless otherwise noted
4. Copernicium is reported to be the only metal known to be a gas at room temperature.
5. 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".
6. 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.
7. 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.
8. 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.
9. Boron 0.13; silicon 0.22; germanium 0.278; amorphous arsenic 0.27; antimony 0.25; tellurium ~0.2.
10. Graphitic carbon 0.25; ; black phosphorus 0.30; sulfur 0.287; amorphous selenium 0.32; amorphous iodine ~0.
11. At atmospheric pressure, for elements with known structures
12. 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 among the elements.
13. Metals have electrical conductivity values of from 6.9 × 10 S•cm for manganese to 6.3 × 10 for silver.
14. 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.
15. Nonmetals have electrical conductivity values of from ~10 S•cm for the elemental gases to 3 × 10 in graphite.
16. Mott and Davis note however that 'liquid europium has a negative temperature coefficient of resistance' i.e. that conductivity increases with rising temperature
17. At or near room temperature
18. 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'.
19. Phosphorus is known to form a carbide in thin films.
20. See, for example, the sulfates of the transition metals, the lanthanides and the actinides.
21. Sulfates of osmium have not been characterized with any great degree of certainty.
22. Common metalloids: Boron is reported to be capable of forming an oxysulfate (BO)₂SO₄, a bisulfate B(HSO₄)₃ and a sulfate B₂(SO₄)₃. 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(SO₄)₂ (d 200 °C). Arsenic forms oxide sulfates As₂O(SO₄)₂ (= As₂O₃.2SO₃) and As₂(SO₄)₃ (= As₂O₃.3SO₃). Antimony forms a sulfate Sb₂(SO₄)₃ and an oxysulfate (SbO)₂SO₄. Tellurium forms an oxide sulfate Te₂O₃(SO)₄. Less common: Polonium forms a sulfate Po(SO₄)₂. It has been suggested that the astatine cation forms a weak complex with sulfate ions in acidic solutions.
23. Hydrogen forms hydrogen sulfate H₂SO₄. Carbon forms (a blue) graphite hydrogen sulfate C
    ₂₄HSO
    ₄ • 2.4H₂SO₄. Nitrogen forms nitrosyl hydrogen sulfate (NO)HSO₄ and nitronium (or nitryl) hydrogen sulfate (NO₂)HSO₄. There are indications of a basic sulfate of selenium SeO₂.SO₃ or SeO(SO₄). Iodine forms a polymeric yellow sulfate (IO)₂SO₄.
24. layer-lattice types often reversibly so
25. 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."
26. 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.
27. Fluorine can be found in its elemental form, as an occlusion in the mineral antozonite
28. 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." 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 different.'

Citations

1. Mendeléeff 1897, p. 274
2. Brinkley 1945, p. 378
3. Glinka 1965, p. 88
4. Eby et al. 1943, p. 404
5. Booth & Bloom 1972, p. 426
6. ^ Cox 2004, p. 27
7. Huheey, Keiter & Keiter 1993, p. 28
8. ^ Kneen, Rogers & Simpson, 1972, p. 263. Columns 2 (metals) and 4 (nonmetals) are sourced from this reference unless otherwise indicated.
9. Russell & Lee 2005, p. 147
10. ^ Rochow 1966, p. 4
11. Pottenger & Bowes 1976, p. 138
12. Askeland, Fulay & Wright 2011, p. 806
13. Born & Wolf 1999, p. 746
14. Lagrenaudie 1953
15. Rochow 1966, pp. 23, 25
16. Burakowski & Wierzchoń 1999, p. 336
17. Olechna & Knox 1965, pp. A991‒92
18. Stoker 2010, p. 62
19. Chang 2002, p. 304. Chang speculates that the melting point of francium would be about 23 °C.
20. New Scientist 1975; Soverna 2004; Eichler, Aksenov & Belozeroz et al. 2007; Austen 2012
21. Hunt 2000, p. 256
22. Sisler 1973, p. 89
23. Hérold 2006, pp. 149–150
24. Russell & Lee 2005
25. Legit, Friák & Šob 2010, p. 214118-18
26. Manson & Halford 2006, pp. 378, 410
27. ^ McQuarrie & Rock 1987, p. 85
28. Chung 1987; Godfrin & Lauter 1995
29. Cambridge Enterprise 2013
30. Faraday 1853, p. 42; Holderness & Berry 1979, p. 255
31. Partington 1944, p. 405
32. Regnault 1853, p. 208
33. Christensen 2012, p. 14
34. Gschneidner 1964, pp. 292‒93.
35. Qin et al. 2012, p. 258
36. Hopcroft, Nix & Kenny 2010, p. 236
37. Greaves et al. 2011, p. 826
38. Brassington et al. 1980
39. Martienssen & Warlimont 2005, p. 100
40. Witczak 2000, p. 823
41. Marlowe 1970, p. 6;Slyh 1955, p. 146
42. Klein & Cardinale 1992, pp. 184‒85
43. Appalakondaiah et al. 2012, pp. 035105‒6
44. Sundara Rao 1950; Sundara Rao 1954; Ravindran 1998, pp. 4897‒98
45. Lindegaard & Dahle 1966, p. 264
46. Leith 1966, pp. 38‒39
47. Donohoe 1982; Russell & Lee 2005
48. Gupta et al. 2005, p. 502
49. Walker, Newman & Enache 2013, p. 25
50. Wiberg 2001, p. 143
51. Batsanov & Batsanov 2012, p. 275
52. Clementi & Raimondi 1963; Clementi, Raimondi & Reinhardt 1967
53. Addison 1964; Donohoe 1982
54. Vernon 2013, p. 1704
55. Parish 1977, pp. 34, 48, 112, 142, 156, 178
56. ^ Emsley 2001, p. 12
57. Russell 1981, p. 628
58. Herzfeld 1927; Edwards 2000, pp. 100–103
59. Edwards 1999, p. 416
60. Edwards & Sienko 1983, p. 695
61. ^ Edwards & Sienko 1983, p. 691
62. Edwards et al. 2010
63. Desai, James & Ho 1984, p. 1160; Matula 1979, p. 1260
64. Choppin & Johnsen 1972, p. 351
65. Schaefer 1968, p. 76; Carapella 1968, p. 30
66. Glazov, Chizhevskaya & Glagoleva 1969 p. 86
67. Kozyrev 1959, p. 104
68. Chizhikov & Shchastlivyi 1968, p. 25
69. Bogoroditskii & Pasynkov 1967, p. 77; Jenkins & Kawamura 1976, p. 88
70. Rao & Ganguly 1986
71. Mott & Davis 2012, p. 177
72. Antia 1998
73. Cverna 2002, p.1
74. Cordes & Scaheffer 1973, p. 79
75. Hill & Holman 2000, p. 42
76. Tilley 2004, p. 487
77. Russell & Lee 2005, p. 466
78. Orton 2004, pp. 11–12
79. Zhigal'skii & Jones 2003, p. 66: 'Bismuth, antimony, arsenic and graphite are considered to be semimetals ... In bulk semimetals ... the resistivity will increase with temperature ... to give a positive temperature coefficient of resistivity ...'
80. Jauncey 1948, p. 500: 'Nonmetals mostly have negative temperature coefficients. For instance, carbon ... resistance 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.'
81. Reynolds 1969, pp. 91–92
82. ^ Wilson 1966, p. 260
83. Wittenberg 1972, p. 4526
84. Habashi 2003, p. 73
85. Bailar et al. 1989, p. 742
86. Hiller & Herber 1960, inside front cover; p. 225
87. Beveridge et al. 1997, p. 185
88. ^ Young & Sessine 2000, p. 849
89. Bailar et al. 1989, p. 417
90. Metcalfe, Williams & Castka 1966, p. 72
91. Chang 1994, p. 311
92. Pauling 1988, p. 183
93. Mann et al. 2000, p. 2783
94. Chedd 1969, pp. 24–25
95. Adler 1969, pp. 18–19
96. Hultgren 1966, p. 648
97. Bassett et al. 1966, p. 602
98. Rochow 1966, p. 34
99. Martienssen & Warlimont 2005, p. 257
100. Sidorov 1960
101. Brasted 1974, p. 814
102. Atkins 2006 et al., pp. 8, 122–23
103. Rao 2002, p. 22
104. Wickleder, Pley & Büchner 2006; Betke & Wickleder 2011
105. Cotton 1994, p. 3606
106. Keogh 2005, p. 16
107. Raub & Griffith 1980, p. 167
108. Nemodruk & Karalova 1969, p. 48
109. Sneed 1954, p. 472; Gillespie & Robinson 1959, p. 407
110. Zuckerman & Hagen 1991, p. 303
111. Sanderson 1967, p. 178
112. Iler 1979, p. 190
113. Sanderson 1960, p. 162; Greenwood & Earnshaw 2002, p. 387
114. Mercier & Douglade 1982
115. Douglade & Mercier 1982
116. Wiberg 2001, p. 764
117. Wickleder 2007, p. 350
118. Bagnall 1966, pp. 140−41
119. Berei & Vasáros 1985, pp. 221, 229
120. Wiberg 2001, p. 795
121. Lidin 1996, pp. 266, 270; Brescia et al. 1975, p. 453
122. Greenwood & Earnshaw 2002, p. 786
123. Furuseth et al. 1974
124. Holtzclaw, Robinson & Odom 1991, pp. 706–07; Keenan, Kleinfelter & Wood 1980, pp. 693–95
125. Kneen, Rogers & Simpson 1972, p. 278
126. Heslop & Robinson 1963, p. 417
127. Rochow 1966, pp. 28–29
128. Bagnall 1966, pp. 108, 120; Lidin 1996, passim
129. ^ Smith 1921, p. 295; Sidgwick 1950, pp. 605, 608; Dunstan 1968, pp. 408, 438
130. Dunstan 1968, pp. 312, 408
131. Georgievskii 1982, p. 58
132. Lide & Frederikse 1998, p. 14–6
133. Hem 1985, p. 7
134. Perkins 1998, p. 350
135. Sanderson 2012
136. Brown et al. 2009, p. 137
137. Bresica et al. 1975, p. 137
138. Jansen 2005
139. ^ Russell & Lee 2005, p. 246
140. Russell & Lee 2005, p. 244–5
141. Donohoe 1982, pp. 191–196; Russell & Lee 2005, pp. 244–247
142. Jackson 2000
143. Stoye 2014
144. Witt 1991; Endicott 1998
145. Dumé 2003
146. Benedict et al. 1946, p. 19
147. Noddack 1934, p. 653
148. Sacks 2001, p. 205: 'This story was told by Glenn Seaborg when he was presenting his recollections at a conference in November 1997.'
149. Hecker, Siegfried S. (2000). "Plutonium and its alloys: from atoms to microstructure" (PDF). Los Alamos Science. 26: 290–335. Archived (PDF) from the original on February 24, 2009. Retrieved February 15, 2009.
150. Tsiovkin, Yu.Yu.; Lukoyanov, A.V.; Shorikov, A.O.; Tsiovkina, L.Yu.; Dyachenko, A.A.; Bystrushkin, V.B.; Korotin, M.A.; Anisimov, V.I.; Dremov, V.V. (2011). "Electrical resistivity of pure transuranium metals under pressure". Journal of Nuclear Materials. 413 (1): 41–46. doi:10.1016/j.jnucmat.2011.03.053.
151. Dalhouse University 2015; White et al. 2015
152. ^ DuPlessis 2007, p. 133
153. Gösele & Lehmann 1994, p. 19
154. Chen, Lee & Bosman 1994
155. ^ Kovalev et al. 2001, p. 068301-1
156. Mikulec, Kirtland & Sailor 2002
157. Bychkov 2012, pp. 20–21; see also Lazaruk et al. 2007
158. Slezak 2014
159. Wiberg 2001, p. 758; see also Fraden 1951
160. Sacks 2001, p. 204
161. Sacks 2001, pp. 204–205
162. ^ Cerkovnik & Plesničar 2013, p. 7930
163. Emsley 1994, p. 1910
164. ^ Wiberg 2001, p. 497
165. Cross, Saunders & Prinzbach; Chemistry Views 2015
166. Sun, Xu & Gao 2013; Anthony 2013
167. Nakao 1992

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