where do noble metals tend to be located on the table ?

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Where do the noble metals tend to be located on the table – Brainly
Where do the noble metals tend to be located on the table. Advertisement. Rahl. Noble gases are nonmetals. Nevertheless, noble gases are located in Group VIIIA, which is the last vertical column in the Periodic Table. Advertisement. Advertisement.

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Where do the noble metals tend to be located on the table
Where do the noble metals tend to be located on the table – 12498771. CHRISWELLIE1768 CHRISWELLIE1768 04/16/2019 Chemistry High School answered Where do the noble metals tend to be located on the table 1 See answer Advertisement Advertisement …

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Noble metal – Wikipedia
Meaning and history. While noble metal lists can differ, they tend to cluster around the six platinum group metals (ruthenium, rhodium, palladium, osmium, iridium, platinum) plus gold.. In addition to this term’s function as a compound noun, there are circumstances where noble is used as an adjective for the noun metal.A galvanic series is a hierarchy of metals (or other electrically …

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Where are Metals located on the Periodic Table (With Images)
The highly reactive metals are located on the left bottom corner of the Periodic table. They are the Alkali metals of group 1. In 1st group, as we move down from top to bottom, the reactive of metals increases. Thus the bottom most element of group 1 (i.e francium) is the most reactive metal on the Periodic table.

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Noble Metal | Definition, List, & Facts | Britannica
noble metal, any of several metallic chemical elements that have outstanding resistance to oxidation, even at high temperatures; the grouping is not strictly defined but usually is considered to include rhenium, ruthenium, rhodium, palladium, silver, osmium, iridium, platinum, and gold; i.e., the metals of groups VIIb, VIII, and Ib of the second and third transition series of the periodic table. Mercury and copper are sometimes included as noble metals. Silver and gold, which with copper are …

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Where do the noble metals tend to be located on the table
The noble gases are a group of elements in the periodic table. They are located to the far right of the periodic table and make up the eighteenth column. Elements in the noble gas family have atoms with a full outer shell of electrons. They are also called the inert gases. What elements are noble gases? Explanation: Answer from: Quest SHOW ANSWER

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Where Do The Noble Metals Tend To Be Located On The Table …
where do the noble metals tend to be located on the table. where are the noble metals located on the periodic table. where are noble metals found on the periodic table. what are noble metals give one example. what are noble metals why are they used to make ornaments. Noble Metal Catalyst.

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Where are Nonmetals located on the Periodic Table? (+Images)
There are 18 nonmetals on the Periodic table. All these nonmetals are located on the upper right corner of the Periodic table ( Hydrogen is located on the left top corner) In the above image, the nonmetals are represented in yellow color. [ Note: Astatine (atomic number 85) shows characteristics of nonmetals (halogens) as well as metalloids.

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Where do the radioactive elements tend to be located on the table …
Actinium (Ac) at atomic number 89 and lawrencium (Lr) at atomic number 103 make up the first fifteen elements that make up the actinide family. Hence, radioactive elements tend to be located on the actinide series of the periodic table. #SPJ2 Advertisement Answer 4 people found it helpful garimaupreti02 Explanation: Actinide Series of Metals

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Post-transition and related metals in the periodic table
Elements classified as post-transition metals by Masterton, Hurley and Neth:[1] Ga, In, Tl, Sn, Pb, Bi
Also recognised by Huheey, Keiter and Keiter:[2] Al, Ge, Sb, Po; and by Cox:[3] Zn, Cd, Hg
Also recognised by Deming:[4] Cu, Ag, Au (but he counted Al and groups 1 and 2 as ‘light metals’)[n 1]
Also recognised by Scott & Kanda:[8] Pt
Also recognised by King:[9] As, Se, Te
Elements that might be post-transition metals: At, Cn, Nh, Fl, Mc, Lv, Ts
Also shown is the traditional dividing line between metals and nonmetals. The elements otherwise commonly recognised as metalloids (B, Si Ge, As, Sb, Te) are found to either side of this line.
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The metallic elements in the periodic table located between the transition metals and the chemically weak nonmetallic metalloids have received many names in the literature, such as post-transition metals, poor metals, other metals, p-block metals and chemically weak metals; none have been recommended by IUPAC. The most common name, post-transition metals, is generally used in this article. Depending on where the adjacent sets of transition metals and metalloids are judged to begin and end, there are at least five competing proposals for which elements to count as post-transition metals: the three most common contain six, ten and thirteen elements, respectively (see image). All proposals include gallium, indium, tin, thallium, lead, and bismuth.
Physically, these metals are soft (or brittle), have poor mechanical strength, and usually have melting points lower than those of the transition metals. Being close to the metal-nonmetal border, their crystalline structures tend to show covalent or directional bonding effects, having generally greater complexity or fewer nearest neighbours than other metallic elements.
Chemically, they are characterised—to varying degrees—by covalent bonding tendencies, acid-base amphoterism and the formation of anionic species such as aluminates, stannates, and bismuthates (in the case of aluminium, tin, and bismuth, respectively). They can also form Zintl phases (half-metallic compounds formed between highly electropositive metals and moderately electronegative metals or metalloids).
Contents
1 Applicable elements
2 Rationale
3 Descriptive chemistry
3.1 Group 10
3.2 Group 11
3.3 Group 12
3.4 Group 13
3.5 Group 14
3.6 Group 15
3.7 Group 16
3.8 Group 17
3.9 Group 18
4 Aliases and related groupings
4.1 B-subgroup metals
4.1.1 Pseudo metals and hybrid metals
4.2 Base metals
4.3 Borderline metals
4.4 Chemically weak metals
4.5 Frontier metals
4.6 Fusible metals
4.7 Heavy metals (of low melting point)
4.8 Less typical metals
4.9 Metametals
4.10 Ordinary metals
4.11 Other metals
4.12 p-block metals
4.13 Peculiar metals
4.14 Poor metals
4.15 Post-transition metals
4.16 Semimetals
4.17 Soft metals
4.18 Transition metals
5 Notes
6 Sources
7 Further reading
Applicable elements[edit]
Scatter plot of electronegativity values and melting points for metals (up to fermium, element 100) and some borderline elements (Ge, As, Se, Sb, Te, At). Elements categorised by some authors as post-transition metals are distinguished by their relatively high electronegativity values, and relatively low melting points (Pt is anomalous in this regard). High electronegativity corresponds to increasing nonmetallic character;[10] low melting temperature corresponds to weaker cohesive forces between atoms and reduced mechanical strength.[11] The geography of the plot broadly matches that of the periodic table. Starting from the bottom left, and proceeding clockwise, the alkali metals are followed by the heavier alkaline earth metals; the rare earths and actinides (Sc, Y and the lanthanides being here treated as rare earths); transition metals with intermediate electronegativity values and melting points; the refractory metals; the platinum group metals; and the coinage metals leading and forming a part of the post-transition metals. The increased electronegativity of Be and Mg and the higher melting point of Be distances these light alkaline earth metals from their heavier congeners. This separation extends to other differences in physical and chemical behaviour between the light and heavier alkaline earth metals.[n 2]
Usually included in this category are the group 13–15 metals in periods 4–6: gallium, indium and thallium; tin and lead; and bismuth. Other elements sometimes included are platinum (usually considered to be a transition metal); the group 11 metals copper, silver and gold (which are usually considered to be transition metals); the group 12 metals zinc, cadmium and mercury (which are otherwise considered to be transition metals); and aluminium, germanium, arsenic, selenium, antimony, tellurium, and polonium (of which germanium, arsenic, antimony, and tellurium are usually considered to be metalloids). Astatine, which is usually classified as a nonmetal or a metalloid, has been predicted to have a metallic crystalline structure. If so, it would be a post-transition metal. Elements 112–118 (copernicium, nihonium, flerovium, moscovium, livermorium, tennessine, and oganesson) may be post-transition metals; insufficient quantities of them have been synthesized to allow sufficient investigation of their actual physical and chemical properties.
Which elements start to be counted as post-transition metals depends, in periodic table terms, on where the transition metals are taken to end.[n 3] In the 1950s, most inorganic chemistry textbooks defined transition elements as finishing at group 10 (nickel, palladium and platinum), therefore excluding group 11 (copper, silver and gold), and group 12 (zinc, cadmium and mercury). A survey of chemistry books in 2003 showed that the transition metals ended at either group 11 or group 12 with roughly equal frequency.[15] Where the post-transition metals end depends on where the metalloids or nonmetals start. Boron, silicon, germanium, arsenic, antimony and tellurium are commonly recognised as metalloids; other authors treat some or all of these elements as nonmetals. Arsenic, selenium, and tellurium, though lying to the right of the stairstep line, have occasionally been included as post-transition metals.[9]
Rationale[edit]
The diminished metallic nature of the post-transition metals is largely attributable to the increase in nuclear charge going across the periodic table, from left to right.[16] The increase in nuclear charge is partially offset by an increasing number of electrons but as these are spatially distributed each extra electron does not fully screen each successive increase in nuclear charge, and the latter therefore dominates.[17] With some irregularities, atomic radii contract, ionisation energies increase,[16] fewer electrons become available for metallic bonding,[18] and ions [become] smaller and more polarizing and more prone to covalency.[19] This phenomenon is more evident in period 4–6 post-transition metals, due to inefficient screening of their nuclear charges by their d10 and (in the case of the period 6 metals) f14 electron configurations;[20] the screening power of electrons decreases in the sequence s > p > d > f. The reductions in atomic size due to the interjection of the d- and f-blocks are referred to as, respectively, the ‘scandide’ or ‘d-block contraction’,[n 4] and the ‘lanthanide contraction’.[21] Relativistic effects also increase the binding energy, and hence ionisation energy, of the electrons in the 6s shell in gold and mercury, and the 6p shell in subsequent elements of period 6.[22]
Descriptive chemistry[edit]
This section outlines relevant physical and chemical properties of the elements typically or sometimes classified as post-transition metals. For complete profiles, including history, production, specific uses, and biological roles and precautions, see the main article for each element. Abbreviations: MH—Mohs hardness; BCN—bulk coordination number.[n 5]
Group 10[edit]
Main article: Platinum
Platinum is a moderately hard metal (MH 3.5) of low mechanical strength, with a close-packed face-centred cubic structure (BCN 12). Compared to other metals in this category, it has an unusually high melting point (2042 K v 1338 for gold). Platinum is more ductile than gold, silver or copper, thus being the most ductile of pure metals, but it is less malleable than gold. Like gold, platinum is a chalcophile element in terms of its occurrence in the Earth’s crust, preferring to form covalent bonds with sulfur.[25] It behaves like a transition metal in its preferred oxidation states of +2 and +4. There is very little evidence of the existence of simple metal ions in aqueous media;[26] most platinum compounds are (covalent) coordination complexes.[27] The oxide (PtO2) is amphoteric, with acidic properties predominating; it can be fused with alkali hydroxides (MOH; M = Na, K) or calcium oxide (CaO) to give anionic platinates, such as red Na2PtO3 and green K2PtO3. The hydrated oxide can be dissolved in hydrochloric acid to give the hexachlormetallate(IV), H2PtCl6.[28]
Like gold, which can form compounds containing the −1 auride ion, platinum can form compounds containing platinide ions, such as the Zintl phases BaPt, Ba3Pt2 and Ba2Pt, being the first (unambiguous) transition metal to do so.[29]
Darmstadtium should be similar to its lighter homologue platinum. It is expected to have a close-packed body-centered cubic structure. It should be a very dense metal, with a density of 26–27 g/cm3 surpassing all stable elements. Darmstadtium chemistry is expected to be dominated by the +2 and +4 oxidation states, similar to platinum. Darmstadtium(IV) oxide (DsO2) should be amphoteric, and darmstadtium(II) oxide (DsO) basic, exactly analogous to platinum. There should also be a +6 oxidation state, similar to platinum. Darmstadtium should be a very noble metal: the standard reduction potential for the Ds2+/Ds couple is expected to be +1.7 V, more than the +1.52 V for the Au3+/Au couple.
Group 11[edit]
Main article: Group 11 element
The group 11 metals are typically categorised as transition metals given they can form ions with incomplete d-shells. Physically, they have the relatively low melting points and high electronegativity values associated with post-transition metals. The filled d subshell and free s electron of Cu, Ag, and Au contribute to their high electrical and thermal conductivity. Transition metals to the left of group 11 experience interactions between s electrons and the partially filled d subshell that lower electron mobility.[30] Chemically, the group 11 metals in their +1 valence states show similarities to other post-transition metals;[31] they are occasionally classified as such.[32]
Copper
Silver
Gold
Copper is a soft metal (MH 2.5–3.0)[33] with low mechanical strength.[34] It has a close-packed face-centred cubic structure (BCN 12).[35] Copper behaves like a transition metal in its preferred oxidation state of +2. Stable compounds in which copper is in its less preferred oxidation state of +1 (Cu2O, CuCl, CuBr, CuI and CuCN, for example) have significant covalent character.[36] The oxide (CuO) is amphoteric, with predominating basic properties; it can be fused with alkali oxides (M2O; M = Na, K) to give anionic oxycuprates (M2CuO2).[37] Copper forms Zintl phases such as Li7CuSi2[38] and M3Cu3Sb4 (M = Y, La, Ce, Pr, Nd, Sm, Gd, Tb, Dy, Ho, or Er).[39]
Silver is a soft metal (MH 2.5–3)[40] with low mechanical strength.[41] It has a close-packed face-centred cubic structure (BCN 12).[42] The chemistry of silver is dominated by its +1 valence state in which it shows generally similar physical and chemical properties to compounds of thallium, a main group metal, in the same oxidation state.[43] It tends to bond covalently in most of its compounds.[44] The oxide (Ag2O) is amphoteric, with basic properties predominating.[45] Silver forms a series of oxoargentates (M3AgO2, M = Na, K, Rb).[46] It is a constituent of Zintl phases such as Li2AgM (M = Al, Ga, In, Tl, Si, Ge, Sn or Pb)[47] and Yb3Ag2.[48]
Gold is a soft metal (MH 2.5–3)[49] that is easily deformed.[50] It has a close-packed face-centred cubic structure (BCN 12).[42] The chemistry of gold is dominated by its +3 valence state; all such compounds of gold feature covalent bonding,[51] as do its stable +1 compounds.[52] Gold oxide (Au2O3) is amphoteric, with acidic properties predominating; it forms anionic hydroxoaurates M[Au(OH)4], where M = Na, K, ½Ba, Tl; and aurates such as NaAuO2.[53] Gold is a constituent of Zintl phases such as M2AuBi (M = Li or Na);[54] Li2AuM (M = In, Tl, Ge, Pb, Sn)[55] and Ca5Au4.[48]
Roentgenium is expected to be similar to its lighter homologue gold in many ways. It is expected to have a close-packed body-centered cubic structure. It should be a very dense metal, with its density of 22–24 g/cm3 being around that of osmium and iridium, the densest stable elements. Roentgenium chemistry is expected to be dominated by the +3 valence state, similarly to gold, in which it should similarly behave as a transition metal. Roentgenium oxide (Rg2O3) should be amphoteric; stable compounds in the −1, +1, and +5 valence states should also exist, exactly analogous to gold. Roentgenium is similarly expected to be a very noble metal: the standard reduction potential for the Rg3+/Rg couple is expected to be +1.9 V, more than the +1.52 V for the Au3+/Au couple. The [Rg(H2O)2]+ cation is expected to be the softest among the metal cations. Due to relativistic stabilisation of the 7s subshell, roentgenium is expected to have a full s-subshell and a partially filled d-subshell, instead of the free s-electron and full d-subshell of copper, silver, and gold.
Group 12[edit]
Main article: Group 12 element
On the group 12 metals (zinc, cadmium and mercury), Smith[56] observed that, Textbook writers have always found difficulty in dealing with these elements. There is an abrupt and significant reduction in physical metallic character from group 11 to group 12.[57] Their chemistry is that of main group elements.[58] A 2003 survey of chemistry books showed that they were treated as either transition metals or main group elements on about a 50/50 basis.[15][n 6] The IUPAC Red Book notes that although the group 3−12 elements are commonly referred to as the transition elements, the group 12 elements are not always included.[60] The group 12 elements do not satisfy the IUPAC Gold Book definition of a transition metal.[61][n 7]
Zinc
Cadmium
Mercury
Zinc is a soft metal (MH 2.5) with poor mechanical properties.[63] It has a crystalline structure (BCN 6+6) that is slightly distorted from the ideal. Many zinc compounds are markedly covalent in character.[64] The oxide and hydroxide of zinc in its preferred oxidation state of +2, namely ZnO and Zn(OH)2, are amphoteric;[65] it forms anionic zincates in strongly basic solutions.[66] Zinc forms Zintl phases such as LiZn, NaZn13 and BaZn13.[67] Highly purified zinc, at room temperature, is ductile.[68] It reacts with moist air to form a thin layer of carbonate that prevents further corrosion.[69]
Cadmium is a soft, ductile metal (MH 2.0) that undergoes substantial deformation, under load, at room temperature.[70] Like zinc, it has a crystalline structure (BCN 6+6) that is slightly distorted from the ideal. The halides of cadmium, with the exception of the fluoride, exhibit a substantially covalent nature.[71] The oxides of cadmium in its preferred oxidation state of +2, namely CdO and Cd(OH)2, are weakly amphoteric; it forms cadmates in strongly basic solutions.[72] Cadmium forms Zintl phases such as LiCd, RbCd13 and CsCd13.[67] When heated in air to a few hundred degrees, cadmium represents a toxicity hazard due to the release of cadmium vapour; when heated to its boiling point in air (just above 1000 K; 725 C; 1340 F; cf steel ~2700 K; 2425 C; 4400 F),[73] the cadmium vapour oxidizes, ‘with a reddish-yellow flame, dispersing as an aerosol of potentially lethal CdO particles.'[70] Cadmium is otherwise stable in air and in water, at ambient conditions, protected by a layer of cadmium oxide.
Mercury is a liquid at room temperature. It has the weakest metallic bonding of all, as indicated by its bonding energy (61 kJ/mol) and melting point (−39 °C) which, together, are the lowest of all the metallic elements.[74][n 8] Solid mercury (MH 1.5)[75] has a distorted crystalline structure,[76] with mixed metallic-covalent bonding,[77] and a BCN of 6. All of the [Group 12] metals, but especially mercury, tend to form covalent rather than ionic compounds.[78] The oxide of mercury in its preferred oxidation state (HgO; +2) is weakly amphoteric, as is the congener sulfide HgS.[79] It forms anionic thiomercurates (such as Na2HgS2 and BaHgS3) in strongly basic solutions.[80][n 9] It forms or is a part of Zintl phases such as NaHg and K8In10Hg.[81] Mercury is a relatively inert metal, showing little oxide formation at room temperature.[82]
Copernicium is expected to be a liquid at room temperature, although experiments have so far not succeeded in determining its boiling point with sufficient precision to prove this. Like its lighter congener mercury, many of its singular properties stem from its closed-shell d10s2 electron configuration as well as strong relativistic effects. Its cohesive energy is even less than that of mercury and is likely only higher than that of flerovium. Solid copernicium is expected to crystallise in a close-packed body-centred cubic structure and have a density of about 14.7 g/cm3, decreasing to 14.0 g/cm3 on melting, which is similar to that of mercury (13.534 g/cm3). Copernicium chemistry is expected to be dominated by the +2 oxidation state, in which it would behave like a post-transition metal similar to mercury, although the relativistic stabilisation of the 7s orbitals means that this oxidation state involves giving up 6d rather than 7s electrons. A concurrent relativistic destabilisation of the 6d orbitals should allow higher oxidation states such as +3 and +4 with electronegative ligands, such as the halogens. A very high standard reduction potential of +2.1 V is expected for the Cn2+/Cn couple. In fact, bulk copernicium may even be an insulator with a band gap of 6.4±0.2 V, which would make it similar to the noble gases such as radon, though copernicium has previously been predicted to be a semiconductor or a noble metal instead. Copernicium oxide (CnO) is expected to be predominantly basic.
Group 13[edit]
Main article: Boron group
Aluminium
Gallium
Indium
Thallium
Aluminium sometimes is[83] or is not[3] counted as a post-transition metal. It has a well shielded [Ne] noble gas core rather than the less well shielded [Ar]3d10, [Kr]4d10 or [Xe]4f145d10 core of the post-transition metals. The small radius of the aluminium ion combined with its high charge make it a strongly polarizing species, prone to covalency.[84]
Aluminium in pure form is a soft metal (MH 3.0) with low mechanical strength.[85] It has a close-packed structure (BCN 12) showing some evidence of partially directional bonding.[86][n 10] It has a low melting point and a high thermal conductivity. Its strength is halved at 200 °C, and for many of its alloys is minimal at 300 °C.[88] The latter three properties of aluminium limit its use to situations where fire protection is not required,[89] or necessitate the provision of increased fire protection.[90][n 11] It bonds covalently in most of its compounds;[94] has an amphoteric oxide; and can form anionic aluminates.[66] Aluminium forms Zintl phases such as LiAl, Ca3Al2Sb6, and SrAl2.[95] A thin protective layer of oxide confers a reasonable degree of corrosion resistance.[96] It is susceptible to attack in low pH ( 8.5) pH conditions,[97][n 12] a phenomenon that is generally more pronounced in the case of commercial purity aluminium and aluminium alloys.[103] Given many of these properties and its proximity to the dividing line between metals and nonmetals, aluminium is occasionally classified as a metalloid.[n 13] Despite its shortcomings, it has a good strength-to-weight ratio and excellent ductility; its mechanical strength can be improved considerably with the use of alloying additives; its very high thermal conductivity can be put to good use in heat sinks and heat exchangers;[104] and it has a high electrical conductivity.[n 14] At lower temperatures, aluminium increases its deformation strength (as do most materials) whilst maintaining ductility (as do face-centred cubic metals generally).[106] Chemically, bulk aluminium is a strongly electropositive metal, with a high negative electrode potential.[107][n 15]
Gallium is a soft, brittle metal (MH 1.5) that melts at only a few degrees above room temperature.[109] It has an unusual crystalline structure featuring mixed metallic-covalent bonding and low symmetry[109] (BCN 7 i.e. 1+2+2+2).[110] It bonds covalently in most of its compounds,[111] has an amphoteric oxide;[112] and can form anionic gallates.[66] Gallium forms Zintl phases such as Li2Ga7, K3Ga13 and YbGa2.[113] It is slowly oxidized in moist air at ambient conditions; a protective film of oxide prevents further corrosion.[114]
Indium is a soft, highly ductile metal (MH 1.0) with a low tensile strength.[115][116] It has a partially distorted crystalline structure (BCN 4+8) associated with incompletely ionised atoms.[117] The tendency of indium ‘…to form covalent compounds is one of the more important properties influencing its electrochemical behavior’.[118] The oxides of indium in its preferred oxidation state of +3, namely In2O3 and In(OH)3 are weakly amphoteric; it forms anionic indates in strongly basic solutions.[119] Indium forms Zintl phases such as LiIn, Na2In and Rb2In3.[120] Indium does not oxidize in air at ambient conditions.[116]
Thallium is a soft, reactive metal (MH 1.0), so much so that it has no structural uses.[121] It has a close-packed crystalline structure (BCN 6+6) but an abnormally large interatomic distance that has been attributed to partial ionisation of the thallium atoms.[122] Although compounds in the +1 (mostly ionic) oxidation state are the more numerous, thallium has an appreciable chemistry in the +3 (largely covalent) oxidation state, as seen in its chalcogenides and trihalides.[123] It is the only one of the Group 13 elements to react with air at room temperature, slowly forming the amphoteric oxide Tl2O3.[124][125][126] It forms anionic thallates such as Tl3TlO3, Na3Tl(OH)6, NaTlO2, and KTlO2,[125] and is present as the Tl− thallide anion in the compound CsTl.[127] Thallium forms Zintl phases, such as Na2Tl, Na2K21Tl19, CsTl and Sr5Tl3H.[128]
Nihonium is expected to have a hexagonal close-packed crystalline structure, albeit based on extrapolation from those of the lighter group 13 elements: its density is expected to be around 16 g/cm3. A standard electrode potential of +0.6 V is predicted for the Nh+/Nh couple. The relativistic stabilisation of the 7s electrons is very high and hence nihonium should predominantly form the +1 oxidation state; nevertheless, as for copernicium, the +3 oxidation state should be reachable. Because of the shell closure at flerovium caused by spin-orbit coupling, nihonium is also one 7p electron short of a closed shell and would hence form a −1 oxidation state; in both the +1 and −1 oxidation states, nihonium should show more similarities to astatine than thallium. The Nh+ ion is expected to also have some similarities to the Ag+ ion, particularly in its propensity for complexation. Nihonium oxide (Nh2O) is expected to be amphoteric.
Group 14[edit]
Main article: Carbon group
Germanium
Tin
Lead
Germanium is a hard (MH 6), very brittle semi-metallic element.[129] It was originally thought to be a poorly conducting metal[130] but has the electronic band structure of a semiconductor.[131] Germanium is usually considered to be a metalloid rather than a metal.[132] Like carbon (as diamond) and silicon, it has a covalent tetrahedral crystalline structure (BCN 4).[133] Compounds in its preferred oxidation state of +4 are covalent.[134] Germanium forms an amphoteric oxide, GeO2[135] and anionic germanates, such as Mg2GeO4.[136] It forms Zintl phases such as LiGe, K8Ge44 and La4Ge3.[137]
Tin is a soft, exceptionally[138] weak metal (MH 1.5);[n 16] a 1-cm thick rod will bend easily under mild finger pressure.[138] It has an irregularly coordinated crystalline structure (BCN 4+2) associated with incompletely ionised atoms.[117] All of the Group 14 elements form compounds in which they are in the +4, predominantly covalent, oxidation state; even in the +2 oxidation state tin generally forms covalent bonds.[140] The oxides of tin in its preferred oxidation state of +2, namely SnO and Sn(OH)2, are amphoteric;[141] it forms stannites in strongly basic solutions.[66] Below 13 °C (55.4 °F) tin changes its structure and becomes ‘grey tin’, which has the same structure as diamond, silicon and germanium (BCN 4). This transformation causes ordinary tin to crumble and disintegrate since, as well as being brittle, grey tin occupies more volume due to having a less efficient crystalline packing structure. Tin forms Zintl phases such as Na4Sn, BaSn, K8Sn25 and Ca31Sn20.[142] It has good corrosion resistance in air on account of forming a thin protective oxide layer. Pure tin has no structural uses.[143] It is used in lead-free solders, and as a hardening agent in alloys of other metals, such as copper, lead, titanium and zinc.[144]
Lead is a soft metal (MH 1.5, but hardens close to melting) which, in many cases,[145] is unable to support its own weight.[146] It has a close-packed structure (BCN 12) but an abnormally large inter-atomic distance that has been attributed to partial ionisation of the lead atoms.[122][147] It forms a semi-covalent dioxide PbO2; a covalently bonded sulfide PbS; covalently bonded halides;[148] and a range of covalently bonded organolead compounds such as the lead(II) mercaptan Pb(SC2H5)2, lead tetra-acetate Pb(CH3CO2)4, and the once common, anti-knock additive, tetra-ethyl lead (CH3CH2)4Pb.[149] The oxide of lead in its preferred oxidation state (PbO; +2) is amphoteric;[150] it forms anionic plumbates in strongly basic solutions.[66] Lead forms Zintl phases such as CsPb, Sr31Pb20, La5Pb3N and Yb3Pb20.[151] It has reasonable to good corrosion resistance; in moist air it forms a mixed gray coating of oxide, carbonate and sulfate that hinders further oxidation.[152]
Flerovium is expected to be a liquid metal due to spin-orbit coupling tearing apart the 7p subshell, so that its 7s27p1/22 valence configuration forms a quasi-closed shell similar to those of mercury and copernicium. Solid flerovium should have a face-centered cubic structure and be a rather dense metal, with a density of around 14 g/cm3. Flerovium is expected to have a standard electrode potential of +0.9 V for the Fl2+/Fl couple. Flerovium oxide (FlO) is expected to be amphoteric, forming anionic flerovates in basic solutions.
Group 15[edit]
Main article: Pnictogen
Arsenic
Antimony
Bismuth
Arsenic is a moderately hard (MH 3.5) and brittle semi-metallic element. It is commonly regarded as a metalloid, or by some other authors as either a metal or a non-metal. It exhibits poor electrical conductivity which, like a metal, decreases with temperature. It has a relatively open and partially covalent crystalline structure (BCN 3+3). Arsenic forms covalent bonds with most other elements. The oxide in its preferred oxidation state (As2O3, +3) is amphoteric,[n 17] as is the corresponding oxoacid in aqueous solution (H3AsO3) and congener sulfide (As2S3). Arsenic forms a series of anionic arsenates such as Na3AsO3 and PbHAsO4, and Zintl phases such as Na3As, Ca2As and SrAs3.
Antimony is a soft (MH 3.0) and brittle semi-metallic element. It is commonly regarded as a metalloid, or by some other authors as either a metal or a non-metal. It exhibits poor electrical conductivity which, like a metal, decreases with temperature. It has a relatively open and partially covalent crystalline structure (BCN 3+3). Antimony forms covalent bonds with most other elements. The oxide in its preferred oxidation state (Sb2O3, +3) is amphoteric. Antimony forms a series of anionic antimonites and antimonates such as NaSbO2 and AlSbO4, and Zintl phases such as K5Sb4, Sr2Sb3 and BaSb3.
Bismuth is a soft metal (MH 2.5) that is too brittle for any structural use.[155] It has an open-packed crystalline structure (BCN 3+3) with bonding that is intermediate between metallic and covalent.[156] For a metal, it has exceptionally low electrical and thermal conductivity.[157] Most of the ordinary compounds of bismuth are covalent in nature.[158] The oxide, Bi2O3 is predominantly basic but will act as a weak acid in warm, very concentrated KOH.[159] It can also be fused with potassium hydroxide in air, resulting in a brown mass of potassium bismuthate.[160] The solution chemistry of bismuth is characterised by the formation of oxyanions;[161] it forms anionic bismuthates in strongly basic solutions.[162] Bismuth forms Zintl phases such as NaBi,[163] Rb7In4Bi6[164] and Ba11Cd8Bi14.[165] Bailar et al.[166] refer to bismuth as being, ‘the least metallic metal in its physical properties’ given its brittle nature (and possibly) ‘the lowest electrical conductivity of all metals.'[n 18]
Moscovium is expected to be a quite reactive metal. A standard reduction potential of −1.5 V for the Mc+/Mc couple is expected. This increased reactivity is consistent with the quasi-closed shell of flerovium and the beginning of a new series of elements with the filling of the loosely bound 7p3/2 subshell, and is rather different from the relative nobility of bismuth. Like thallium, moscovium should have a common +1 oxidation state and a less common +3 oxidation state, although their relative stabilities may change depending on the complexing ligands or the degree of hydrolysis. Moscovium(I) oxide (Mc2O) should be quite basic, like that of thallium, while moscovium(III) oxide (Mc2O3) should be amphoteric, like that of bismuth.
Group 16[edit]
Main article: Chalcogen
Selenium
Tellurium
Selenium is a soft (MH 2.0) and brittle semi-metallic element. It is commonly regarded as a nonmetal, but is sometimes considered a metalloid or even a heavy metal. Selenium has a hexagonal polyatomic (CN 2) crystalline structure. It is a semiconductor with a band gap of 1.7 eV, and a photoconductor meaning its electrical conductivity increases a million-fold when illuminated. Selenium forms covalent bonds with most other elements, noting it can form ionic selenides with highly electropositive metals. The common oxide of selenium (SeO3) is strongly acidic. Selenium forms a series of anionic selenites and selenates such as Na2SeO3, Na2Se2O5, and Na2SeO4,[168] as well as Zintl phases such as Cs4Se16.[169]
Tellurium is a soft (MH 2.25) and brittle semi-metallic element. It is commonly regarded as a metalloid, or by some authors either as a metal or a non-metal. Tellurium has a polyatomic (CN 2) hexagonal crystalline structure. It is a semiconductor with a band gap of 0.32 to 0.38 eV. Tellurium forms covalent bonds with most other elements, noting it has an extensive organometallic chemistry and that many tellurides can be regarded as metallic alloys. The common oxide of tellurium (TeO2) is amphoteric. Tellurium forms a series of anionic tellurites and tellurates such as Na2TeO3, Na6TeO6, and Rb6Te2O9 (the last containing tetrahedral TeO2−
4 and trigonal bipyramidal TeO4−
5 anions),[168] as well as Zintl phases such as NaTe3.[169]
Polonium is a radioactive, soft metal with a hardness similar to lead.[170] It has a simple cubic crystalline structure characterised (as determined by electron density calculations) by partially directional bonding,[171] and a BCN of 6. Such a structure ordinarily results in very low ductility and fracture resistance[172] however polonium has been predicted to be a ductile metal.[173] It forms a covalent hydride;[174] its halides are covalent, volatile compounds, resembling those of tellurium.[175] The oxide of polonium in its preferred oxidation state (PoO2; +4) is predominantly basic, but amphoteric if dissolved in concentrated aqueous alkali, or fused with potassium hydroxide in air.[176] The yellow polonate(IV) ion PoO2−
3 is known in aqueous solutions of low Cl‒ concentration and high pH.[177][n 19] Polonides such as Na2Po, BePo, ZnPo, CdPo and HgPo feature Po2− anions;[179] except for HgPo these are some of the more stable of the polonium compounds.[180][n 20]
Livermorium is expected to be less reactive than moscovium. The standard reduction potential of the Lv2+/Lv couple is expected to be around +0.1 V. It should be most stable in the +2 oxidation state; the 7p3/2 electrons are expected to be so weakly bound that the first two ionisation potentials of livermorium should lie between those of the reactive alkaline earth metals magnesium and calcium. The +4 oxidation state should only be reachable with the most electronegative ligands. Livermorium(II) oxide (LvO) should be basic and livermorium(IV) oxide (LvO2) should be amphoteric, analogous to polonium.
Group 17[edit]
Main article: Halogen
Astatine is a radioactive element that has never been seen; a visible quantity would immediately be vaporised due to its intense radioactivity.[182] It may be possible to prevent this with sufficient cooling.[183] Astatine is commonly regarded as a nonmetal,[184] less commonly as a metalloid[185] and occasionally as a metal. Unlike its lighter congener iodine, evidence for diatomic astatine is sparse and inconclusive.[186] In 2013, on the basis of relativistic modelling, astatine was predicted to be a monatomic metal, with a face-centered cubic crystalline structure.[183] As such, astatine could be expected to have a metallic appearance; show metallic conductivity; and have excellent ductility, even at cryogenic temperatures.[187] It could also be expected to show significant nonmetallic character, as is normally the case for metals in, or in the vicinity of, the p-block. Astatine oxyanions AtO−, AtO−
3 and AtO−
4 are known,[188] oxyanion formation being a tendency of nonmetals.[189] The hydroxide of astatine At(OH) is presumed to be amphoteric.[190][n 21] Astatine forms covalent compounds with nonmetals,[193] including hydrogen astatide HAt and carbon tetraastatide CAt4.[194][n 22] At− anions have been reported to form astatides with silver, thallium, palladium and lead.[196] Pruszyński et al. note that astatide ions should form strong complexes with soft metal cations such as Hg2+, Pd2+, Ag+ and Tl3+; they list the astatide formed with mercury as Hg(OH)At.[197]
Tennessine, despite being in the halogen column of the periodic table, is expected to go even further towards metallicity than astatine due to its small electron affinity. The −1 state should not be important for tennessine and its major oxidation states should be +1 and +3, with +3 more stable: Ts3+ is expected to behave similarly to Au3+ in halide media. As such, tennessine oxide (Ts2O3) is expected to be amphoteric, similar to gold oxide and astatine(III) oxide.
Group 18[edit]
Main article: Oganesson
Oganesson is expected to be a very poor noble gas and may even be metallised by its large atomic radius and the weak binding of the easily removed 7p3/2 electrons: certainly it is expected to be a quite reactive element that is solid at room temperature and has some similarities to tin, as one effect of the spin–orbit splitting of the 7p subshell is a partial role reversal of groups 14 and 18. Due to the immense polarisability of oganesson, it is expected that not only oganesson(II) fluoride but also oganesson(IV) fluoride should be predominantly ionic, involving the formation of Og2+ and Og4+ cations. Oganesson(II) oxide (OgO) and oganesson(IV) oxide (OgO2) are both expected to be amphoteric, similar to the oxides of tin.
Aliases and related groupings[edit]
B-subgroup metals[edit]
Superficially, the B-subgroup metals are the metals in Groups IB to VIIB of the periodic table, corresponding to groups 11 to 17 using current IUPAC nomenclature. Practically, the group 11 metals (copper, silver and gold) are ordinarily regarded as transition metals (or sometimes as coinage metals, or noble metals) whereas the group 12 metals (zinc, cadmium, and mercury) may or may not be treated as B-subgroup metals depending on if the transition metals are taken to end at group 11 or group 12. The ‘B’ nomenclature (as in Groups IB, IIB, and so on) was superseded in 1988 but is still occasionally encountered in more recent literature.[198][n 23]
The B-subgroup metals show nonmetallic properties; this is particularly apparent in moving from group 12 to group 16.[200] Although the group 11 metals have normal close-packed metallic structures[201] they show an overlap in chemical properties. In their +1 compounds (the stable state for silver; less so for copper)[202] they are typical B-subgroup metals. In their +2 and +3 states their chemistry is typical of transition metal compounds.[203]
Pseudo metals and hybrid metals[edit]
The B-subgroup metals can be subdivided into pseudo metals and hybrid metals. The pseudo metals (groups 12 and 13, including boron) are said to behave more like true metals (groups 1 to 11) than non-metals. The hybrid metals As, Sb, Bi, Te, Po, At — which other authors would call metalloids — partake about equally the properties of both. The pseudo metals can be considered related to the hybrid metals through the group 14 carbon column.[204]
Base metals[edit]
Mingos[205] writes that while the p-block metals are typical, that are not strongly reducing and that, as such, they are base metals requiring oxidizing acids to dissolve them.
Borderline metals[edit]
Parish[206] writes that, ‘as anticipated’, the borderline metals of groups 13 and 14 have non-standard structures. Gallium, indium, thallium, germanium, and tin are specifically mentioned in this context. The group 12 metals are also noted as having slightly distorted structures; this has been interpreted as evidence of weak directional (i.e. covalent) bonding.[n 24]
Chemically weak metals[edit]
Rayner-Canham and Overton[208] use the term chemically weak metals to refer to the metals close to the metal-nonmetal borderline. These metals behave chemically more like the metalloids, particularly with respect to anionic species formation. The nine chemically weak metals identified by them are beryllium, magnesium, aluminium, gallium, tin, lead, antimony, bismuth, and polonium.[n 25]
Frontier metals[edit]
Vernon[210] uses the term frontier metal to refer to the class of chemically weak metals adjacent to the dividing line between metals. He notes that several of them are further distinguished by a series of…knight’s move relationships, formed between one element and the element one period down and two groups to its right.[211] For example, copper(I) chemistry resembles indium(I) chemistry: both ions are found mostly in solid-state compounds such as CuCl and InCl; the fluorides are unknown for both ions while the iodides are the most stable.[211] The name frontier metal is adapted from Russell and Lee,[212] who wrote that, …bismuth and group 16 element polonium are generally considered to be metals, although they occupy ‘frontier territory’ on the periodic table, adjacent to the nonmetals.
Fusible metals[edit]
Cardarelli,[213] writing in 2008, categorizes zinc, cadmium, mercury, gallium, indium, thallium, tin, lead, antimony and bismuth as fusible metals. Nearly 100 years earlier, Louis (1911)[214] noted that fusible metals were alloys containing tin, cadmium, lead, and bismuth in various proportions, the tin ranging from 10 to 20%.
Heavy metals (of low melting point)[edit]
Van Wert[215] grouped the periodic table metals into a. the light metals; b. the heavy brittle metals of high melting point, c. the heavy ductile metals of high melting point; d. the heavy metals of low melting point (Zn, Cd, Hg; Ga, In, Tl; Ge, Sn; As, Sb, Bi; and Po), and e. the strong, electropositive metals. Britton, Abbatiello and Robins[216] speak of ‘the soft, low melting point, heavy metals in columns lIB, IlIA, IVA, and VA of the periodic table, namely Zn, Cd, Hg; Al, Ga, In, Tl; [Si], Ge, Sn, Pb; and Bi. The Sargent-Welch Chart of the Elements groups the metals into: light metals, the lanthanide series; the actinide series; heavy metals (brittle); heavy metals (ductile); and heavy metals (low melting point): Zn, Cd, Hg, [Cn]; Al, Ga, In, Tl; Ge, Sn, Pb, [Fl]; Sb, Bi; and Po.[217][n 26]
Less typical metals[edit]
Habashi[219] groups the elements into eight major categories: [1] typical metals (alkali metals, alkaline earth metals, and aluminium); [2] lanthanides (Ce–Lu); [3] actinides (Th–Lr); [4] transition metals (Sc, Y, La, Ac, groups 4–10); [5] less typical metals (groups 11–12, Ga, In, Tl, Sn and Pb); [6] metalloids (B, Si, Ge, As, Se, Sb, Te, Bi and Po); [7] covalent nonmetals (H, C, N, O, P, S and the halogens); and [8] monatomic nonmetals (that is, the noble gases).
Metametals[edit]
The metametals are zinc, cadmium, mercury, indium, thallium, tin and lead. They are ductile elements but, compared to their metallic periodic table neighbours to the left, have lower melting points, relatively low electrical and thermal conductivities, and show distortions from close-packed forms.[220] Sometimes beryllium[221] and gallium[222] are included as metametals despite having low ductility.
Ordinary metals[edit]
Abrikosov[223] distinguishes between ordinary metals, and transition metals where the inner shells are not filled. The ordinary metals have lower melting points and cohesive energies than those of the transition metals.[224] Gray[225] identifies as ordinary metals: aluminium, gallium, indium, thallium, nihonium, tin, lead, flerovium, bismuth, moscovium, and livermorium. He adds that, ‘in reality most of the metals that people think of as ordinary are in fact transition metals…’.
Other metals[edit]
As noted, the metals falling between the transition metals and the metalloids on the periodic table are sometimes called other metals (see also, for example, Taylor et al.).[226] ‘Other’ in this sense has the related meanings of, ‘existing besides, or distinct from, that already mentioned'[227] (that is, the alkali and alkaline earth metals, the lanthanides and actinides, and the transition metals); ‘auxiliary’; ‘ancillary, secondary’.[228] According to Gray[229] there should be a better name for these elements than ‘other metals’.
p-block metals[edit]
The p-block metals are the metals in groups 13‒16 of the periodic table. Usually, this includes aluminium, gallium, indium and thallium; tin and lead; and bismuth. Germanium, antimony and polonium are sometimes also included, although the first two are commonly recognised as metalloids. The p-block metals tend to have structures that display low coordination numbers and directional bonding. Pronounced covalency is found in their compounds; the majority of their oxides are amphoteric.[230]
Aluminium is an undisputed p-block element by group membership and its [Ne] 3s2 3p1 electron configuration, but aluminium does not literally come after transition metals unlike p-block metals from period 4 and on. The epithet post-transition in reference to aluminium is a misnomer, and aluminium normally has no d electrons unlike all other p-block metals.
Peculiar metals[edit]
Slater[231] divides the metals ‘fairly definitely, though not perfectly sharply’ into the ordinary metals and the peculiar metals, the latter of which verge on the nonmetals. The peculiar metals occur towards the ends of the rows of the periodic table and include ‘approximately:’ gallium, indium, and thallium; carbon, silicon ‘(both of which have some metallic properties, though we have previously treated them as nonmetals),’ germanium and tin; arsenic, antimony, and bismuth; and selenium ‘(which is partly metallic)’ and tellurium. The ordinary metals have centro-symmetrical crystalline structures[n 27] whereas the peculiar metals have structures involving directional bonding. More recently, Joshua observed that the peculiar metals have mixed metallic-covalent bonding.[233]
Poor metals[edit]
Farrell and Van Sicien[234] use the term poor metal, for simplicity, ‘to denote one with a significant covalent, or directional character.’ Hill and Holman[235] observe that, ‘The term poor metals is not widely used, but it is a useful description for several metals including tin, lead and bismuth. These metals fall in a triangular block of the periodic table to the right of the transition metals. They are usually low in the activity (electrochemical) series and they have some resemblances to non-metals.’ Reid et al. write that ‘poor metals’ is, ‘[A]n older term for metallic elements in Groups 13‒15 of the periodic table that are softer and have lower melting points than the metals traditionally used for tools.'[236]
Post-transition metals[edit]
An early usage of this name is recorded by Deming, in 1940, in his well-known[237] book Fundamental Chemistry.[4] He treated the transition metals as finishing at group 10 (nickel, palladium and platinum). He referred to the ensuing elements in periods 4 to 6 of the periodic table (copper to germanium; silver to antimony; gold to polonium)—in view of their underlying d10 electronic configurations—as post-transition metals.
Semimetals[edit]
In modern use, the term ‘semimetal’ sometimes refers, loosely or explicitly, to metals with incomplete metallic character in crystalline structure, electrical conductivity or electronic structure. Examples include gallium,[238] ytterbium,[239] bismuth,[240] mercury[241] and neptunium.[242] Metalloids, which are in-between elements that are neither metals nor nonmetals, are also sometimes instead called semimetals. The elements commonly recognised as metalloids are boron, silicon, germanium, arsenic, antimony and tellurium. In old chemistry, before the publication in 1789 of Lavoisier’s ‘revolutionary'[243] Elementary Treatise on Chemistry,[244] a semimetal was a metallic element with ‘very imperfect ductility and malleability'[245] such as zinc, mercury or bismuth.
Soft metals[edit]
Scott and Kanda[8] refer to the metals in groups 11 to 15, plus platinum in group 10, as soft metals, excluding the very active metals, in groups 1−3. They note many important non-ferrous alloys are made from metals in this class, including sterling silver, brass (copper and zinc), and bronzes (copper with tin, manganese and nickel).
Transition metals[edit]
Historically, the transition metal series includes those elements of the Periodic Table which ‘bridge the gap’ between the very electropositive alkali and allkaline earth metals and the electronegative non-metals of the groups: nitrogen-phosphorus, oxygen-sulfur, and the halogens.[246] Cheronis, Parsons and Ronneberg[247] wrote that, The transition metals of low melting point form a block in the Periodic Table: those of Groups II ‘b’ [zinc, cadmium, mercury], III ‘b’ [aluminium, gallium, indium, thallium], and germanium, tin and lead in Group IV. These metals all have melting points below 425 °C.[n 28]
Notes[edit]
^ More recent examples of authors who treat Cu, Ag and Au as post-transition metals include Subba Rao & Shafer;[5] Collings;[6] and Temkin.[7]
^ Physical properties: The lighter alkaline earths possess fairly high electrical and thermal conductivities and sufficient strength for structural use. The heavier elements are poor conductors and are too weak and reactive for structural use.[12] Chemical: The lighter alkaline earths show covalent bonding tendencies (Be predominantly; Mg considerably) whereas compounds of the heavier alkaline earths are predominantly ionic in nature; the heavier alkaline earths have more stable hydrides and less stable carbides.[13]
^ A first IUPAC definition states [T]he elements of groups 3–12 are the d-block elements. These elements are also commonly referred to as the transition elements, though the elements of group 12 are not always included. Depending on the inclusion of group 12 as transition metals, the post-transition metals therefore may or may not include the group 12 elements—zinc, cadmium, and mercury. A second IUPAC definition for transition metals states An element whose atom has an incomplete d sub-shell, or which can give rise to cations with an incomplete d sub-shell. Based on this definition one could argue group 12 should be split with mercury and probably also copernicium as transition metals, and zinc and cadmium as post-transition metals. Of relevance is the synthesis of mercury(IV) fluoride, which seemingly establishes mercury as a transition metal. This conclusion has been challenged by Jensen[14] with the argument that HgF4 only exists under highly atypical non-equilibrium conditions (at 4 K) and should best be considered as an exception. Copernicium has been predicted to have (a) an electron configuration similar to that of mercury; and (b) a predominance of its chemistry in the +4 state, and on that basis would be regarded as a transition metal. However, in recent years, doubt has been cast on the synthesis of HgF4 and the possible existence of copernicium(IV), so that group 12 would have only post-transition metals.
^ The scandide contraction refers to the first row transition metals; the d-block contraction is a more general term.
^ Moh’s hardness values are taken from Samsanov,[23] unless otherwise noted; bulk coordination number values are taken from Darken and Gurry,[24] unless otherwise noted.
^ The group 12 metals have been treated as transition metals for reasons of historical precedent, to compare and contrast properties, to preserve symmetry, or for basic teaching purposes.[59]
^ The IUPAC Gold Book defines a transition metal as ‘An element whose atom has an incomplete d sub-shell, or which can give rise to cations with an incomplete d sub-shell.[62]
^ Francium may have a comparably low bonding energy but its melting point of around 8°C is significantly higher than that of mercury, at −39°C.
^ Mercury also forms partially anionic oxomercurates, such as Li2HgO2 and CdHgO4, by heating mixtures of HgO with the relevant cation oxides, including under oxygen pressure (Müller-Buschbaum 1995; Deiseroth 2004, pp. 173, 177, 185–186).
^ The partially directional bonding in aluminium improves its shear strength but means that ultrahigh-purity aluminium cannot maintain work hardening at room temperature.[87]
^ Without the use of thermal insulation and detailed structural design attention,[91] aluminium’s low melting point and high thermal conductivity mitigate against its use, for example, in military ship construction—should a ship burn, the low melting point results in structural collapse; the high thermal conductivity helps spread the fire.[92] Its use in the construction of cargo ships is limited as little or no economic advantage is gained over steel, once the cost and weight of fitting thermal insulation is taken into account.[93]
^ Aluminium can be attacked, for example, by alkaline detergents[98] (including those used in dishwashers);[99] by wet concrete,[100] and by highly acidic foods such as tomatoes, rhubarb or cabbage.[101] It is not attacked by nitric acid.[102]
^ See the list of metalloid lists for references
^ Aluminium wire is used in electrical transmission lines for the distribution of power but, on account of its low breaking strength, is reinforced with a central core of galvanised steel wire.[105]
^ In the absence of protective measures, the relatively high electropositivity of aluminium renders it susceptible to galvanic corrosion when in physical or electrical contact with other metals such as copper or steel, especially when exposed to saline media, such as sea water or wind-blown sea spray.[108]
^ Charles, Crane and Furness write that, ‘Most metals, except perhaps lead and tin, can be alloyed to give [yield] strengths that lie in the upper two-thirds of the low-strength range…'[139]
^ As2O3 is usually regarded as being amphoteric but a few sources say it is (weakly)[153] acidic. They describe its basic properties (its reaction with concentrated hydrochloric acid to form arsenic trichloride) as being alcoholic, in analogy with the formation of covalent alkyl chlorides by covalent alcohols (e.g., R-OH + HCl → RCl + H2O)[154]
^ Which metal has the lowest electrical conductivity is debatable but bismuth is certainly in the lowest cohort; Hoffman[167] refers to bismuth as ‘a poor metal, on the verge of being a semiconductor.’
^ Bagnall[178] writes that the fusion of polonium dioxide with a potassium chlorate/hydroxide mixture yields a bluish solid which, ‘…presumably contains some potassium polonate.’
^ Bagnall[181] noted that the rare-earth polonides have the greatest thermal stability of any polonium compound.
^ Eagleson refers to the OH compound of astatine as hypoastatous acid HAtO;[191] Pimpentel and Spratley give the formula for hypoastatous acid as HOAt.[192]
^ In hydrogen astatide the negative charge is predicted to be on the hydrogen atom,[195] implying that this compound should instead be referred to as astatine hydride (AtH).
^ Greenwood and Earnshaw[199] refer to the B-subgroup metals as post-transition elements: ‘Arsenic and antimony are classed as metalloids or semi-metals and bismuth is a typical B sub-group (post-transition-element) metal like tin and lead.’
^ Aluminium is identified by Parish, along with germanium, antimony and bismuth, as being a metal on the boundary line between metals and non-metals; he suggests that all these elements are ‘probably better classed as metalloids.'[207]
^ Pauling,[209] in contrast, refers to the strong metals in Groups 1 and 2 (that form ionic compounds with ‘the strong nonmetals in the upper right corner of the periodic table.’).
^ Hawkes,[218] attempting to address the question of what is a heavy metal, commented that, ‘Being a heavy metal has little to do with density, but rather concerns chemical properties’. He observed that, ‘It may mean different things to different people, but as I have used, heard and interpreted the term over the last half-century, it refers to metals with insoluble sulfides and hydroxides, whose salts produce colored solutions in water, and whose complexes are usually colored.’ He goes on to note that, ‘The metals I have seen referred to as heavy metals comprise a block of all the metals in Groups 3 to 16 that are in periods 4 and greater. It may also be stated as the transition metals and post-transition metals.
^ On manganese, Slater says, ‘[It] is a very peculiar and anomalous exception to the general order of the elements. It is the only definite metal, far from the nonmetals in the table, which has a complicated structure.'[232]
^ In fact, both aluminium (660.32) and germanium (938.25) have melting points greater than 425°C.
Sources[edit]
Citations
^ Masterton, Hurley & Neth p. 38
^ Huheey, Keiter & Keiter 1993, p. 28
^
a b Cox 2004, p. 186
^
a b Deming 1940, p. 704–715
^ Subba Rao & Shafer 1979, p. 170
^ Collings 1986, p. 5
^ Temkin 2012, pp. 1, 726
^
a b Scott & Kanda 1963, pp. 385−386
^
a b King 1997, p. 397
^ Roher 2001, pp. 2‒3
^ Messler 2006, p. 347
^ Russell & Lee 2005, p. 165
^ Cotton et al. 1999, pp. 111–113; Greenwood & Earnshaw 2002, p. 111–113
^ Jensen 2008
^
a b Jensen 2003, p. 952
^
a b Cox 2004, p. 17
^ Atkins & de Paula 2011, p. 352
^ Greenwood & Earnshaw 1998, pp. 222–3
^ Steele 1966, p. 193
^ Johnson 1970
^ Huheey & Huheey 1972, p. 229; Mason 1988
^ Cox 2004, pp. 20, 186, 188
^ Samsanov 1968
^ Darken & Gurry 1953, pp. 50–53
^ Reith & Shushter 2018, p. 115
^ Van Loon & Barefoot 1991, p. 52
^ Pauling 1988, p. 695
^ Lidin 1996, p. 347; Wiberg, Holleman & Wiberg 2001, p. 1521
^ Karpov, Konuma & Jansen M 2006, p. 839
^ Russell & Lee 2005, p. 302
^ Steele 1966, p. 67
^ Deming 1940, pp. 705–7; Karamad, Tripkovic & Rossmeisl 2014
^ Cheemalapati, Keleher & Li 2008, p. 226
^ Liu & Pecht 2004, p. 54
^ Donohue 1982, p. 222
^ Vanderah 1992, p. 52
^ Lidin 1996, p. 110
^ Slabon et al. 2012
^ Larson et al. 2006, p. 035111-2
^ Schumann 2008, p. 52
^ Braunović 2014, p. 244
^
a b Donohue 1982, p. 222
^ Banthorpe, Gatforde & Hollebone 1968, p. 61; Dillard & Goldberg 1971, p. 558
^ Steiner & Campbell 1955, p. 394
^ Lidin 1996, p. 5
^ Klassen & Hoppe 1982; Darriet, Devalette & Lecart 1977; Sofin et al. 2002
^ Goodwin et al. 2005, p. 341
^
a b Köhler & Whangbo 2008
^ Arndt & Ganino 2012, p. 115
^ Goffer 2007, p. 176
^ Sidgwick 1950, p. 177
^ Pauling 1988, p. 698
^ Lidin 1996, p. 21–22
^ Miller et al. 2011, p. 150
^ Fishcher-Bünher 2011, p. 150
^ Smith 1990, p. 113
^ Sorensen 1991, p. 3
^ King 1995, pp. xiii, 273–288; Cotton et al. 1999, pp. ix, 598; Massey 2000, pp. 159–176
^ Young et al. 1969; Geffner 1969; Jensen 2003
^ IUPAC 2005, p. 51
^ Crichton 2012, p. 11
^ IUPAC 2006–, transition element entry
^ Schweitzer 2003, p. 603
^ Hutchinson 1964, p. 562
^ Greenwood & Earnshaw 1998, p. 1209; Gupta CK 2002, p. 590
^
a b c d e Rayner-Canham & Overton 2006, p. 30
^
a b Kneip 1996, p. xxii
^ Russell & Lee 2005, p. 339
^ Sequeira 2013, p. 243
^
a b Russell & Lee 2005, p. 349
^ Borsari 2005, p. 608
^ Dirkse 1986, pp. 287–288, 296; Ivanov-Emin, Misel’son & Greksa 1960
^ Wanamaker & Pennington 1921, p. 56
^ Rayner-Canham 2006, p. 570; Chambers & Holliday 1975, p. 58; Wiberg, Holleman & Wiberg 2001, p. 247; Aylward & Findlay 2008, p. 4
^ Poole 2004, p. 821
^ Mittemeijer 2010, p. 138
^ Russell & Lee 2005, pp. 1–2; 354
^ Rayner-Canham 2006, p. 567
^ Moeller 1952, pp. 859, 866
^ Cooney & Hall 1966, p. 2179
^ Deiseroth 2008, pp. 179‒180; Sevov 1993
^ Russell & Lee 2005, p. 354
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^ Kneen, Rogers & Simpson 2004, p. 370; Cox 2004, p. 199
^ Gerard & King 1968, p. 16; Dwight 1999, p. 2
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^ Ogata, Li & Yip 2002; Russell & Lee 2005, p. 360; Glaeser 1992, p. 224
^ Lyons 2004, p. 170
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^ Polemear 2006, p. 184
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^ Ramroth 2006, p. 6; US Dept. of Transportation, Maritime Administration 1987, pp. 97, 358
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^ Cooper 1968, p. 25; Henderson 2000, p. 5
^ Kauzlarich 2005, pp. 6009–10
^ Dennis & Such 1993, p. 391
^ Cramer & Covino 2006, p. 25
^ Hinton & Dobrota 1978, p. 37
^ Holman & Stone 2001, p. 141
^ Hurd 2005, p. 4-15
^ Vargel 2004, p. 580
^ Hill & Holman 2000, p. 276
^ Russell & Lee 2005, p. 360
^ Clegg & Dovaston 2003, p. 5/5
^ Liptrot 2001, p. 181
^ Kent 1993, pp. 13–14
^ Steele 1966, p. 60
^ Davis 1999, p. 75–7
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a b Russell & Lee 2005, p. 387
^ Driess 2004, p. 151; Donohue 1982, p. 237
^ Walker, Enache & Newman 2013, p. 38
^ Atkins et al. 2006, p. 123
^ Corbett 1996, p. 161
^ Eranna 2012, p. 67
^ Chandler 1998, p. 59
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a b Russell & Lee 2005, p. 389
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a b Evans 1966, p. 129–130
^ Liang, King & White 1968, p. 288
^ Busev 1962, p. 33; Liang, King & White 1968, p. 287; Solov’eva et al. 1973, p. 43; Greenwood & Earnshaw 1998, p. 226; Leman & Barron 2005, p. 1522
^ Kneip 1996, p. xxii; Corbett 1996, pp. 153, 158
^ Russell & Lee 2005, p. 390
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a b Wells 1985, p. 1279–80
^ Howe 1968a, p. 709; Taylor & Brothers 1993, p. 131; Lidin 1996, p. 410; Tóth & Győri 2005, pp. 4, 6–7
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a b Bashilova & Khomutova 1984, p. 1546
^ Ropp 2012, p. 484
^ King & Schleyer 2004, p. 19
^ Corbett 1996, p. 153; King 2004, p. 199
^ Wiberg, Holleman & Wiberg 2001, p. 894
^ Haller 2006, p. 3
^ Russell & Lee 2005, p. 399
^ Ryan 1968, p. 65
^ Wiberg, Holleman & Wiberg 2001, p. 895
^ Abd-El-Aziz et al. 2003, p. 200
^ Cooper 1968, pp. 28–9
^ Ropp 2012, p. 405
^ Corbett 1996, p. 143
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a b Russell & Lee 2005, p. 405
^ Charles, Crane & Furness 1997, pp. 49, 57
^ Rayner-Canham 2006, pp. 306, 340
^ Wiberg, Holleman & Wiberg 2001, p. 247
^ Corbett 1996, p. 143; Cotton et al. 1999, pp. 99, 122; Kauzlarich 2005, p. 6009
^ Russell & Lee 2005, pp. 402, 405
^ Russell & Lee 2005, p. 402, 407
^ Alhassan & Goodwin 2005, p. 532
^ Schweitzer 2003, p. 695
^ Mackay & Mackay 1989, p. 86; Norman 1997, p. 36
^ Hutchinson 1959, p. 455; Wells 1984, p. 1188; Liu, Knowles & Chang 1995, p. 125; Bharara & Atwood 2005, pp. 2, 4
^ Durrant & Durrant 1970, p. 670; Lister 1998, p. A12; Cox 2004, p. 204
^ Patnaik 2003, p. 474
^ Corbett 1996, pp. 143, 147; Cotton et al. 1999, p. 122; Kauzlarich 2005, p. 6009
^ Russell & Lee 2005, pp. 411, 13
^ Wiberg 2001, pp. 750, 975; Silberberg 2006, p. 314
^ Sidgwick 1950, p. 784; Moody 1991, pp. 248–9, 319
^ Russell & Lee 2005, p. 428
^ Eagleson 1994, p. 282
^ Russell & Lee 2005, p. 427
^ Sidgwick 1937, p. 181
^ Howe 1968, p. 62
^ Durrant & Durrant 1970, p. 790
^ Wiberg, Holleman & Wiberg 2001, p. 771; McQuarrie, Rock & Gallogly 2010, p. 111
^ Ropp 2012, p. 328
^ Miller, Lee & Choe 2002, p. 14; Aleandri & Bogdanović 2008, p. 326
^ Bobev & Sevov 2002
^ Xia & Bobev 2006
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^ Hoffman 2004
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a b Greenwood & Earnshaw 2002, pp. 781–3
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a b Greenwood & Earnshaw 2002, pp. 762–5
^ Beamer & Maxwell 1946, pp. 1, 31
^ Russell & Lee 2005, p. 431
^ Halford 2006, p. 378
^ Legut, Friák & Šob 2010
^ Wiberg, Holleman & Wiberg 2001, pp. 594; Petrii 2012, p. 754
^ Bagnall 1966, p. 83
^ Bagnall 1966, pp. 42, 61; Wiberg, Holleman & Wiberg 2001, pp. 767–68
^ Schwietzer & Pesterfield pp. 241, 243
^ Bagnall 1962, p. 211
^ Wiberg, Holleman & Wiberg 2001, pp. 283, 595
^ Greenwood & Earnshaw 1998, p. 766
^ Bagnall 1966, p. 47
^ Emsley 2011, p. 58
^
a b Hermann, Hoffmann & Ashcroft 2013, p. 11604–1
^ Hawkes 2010; Holt, Rinehart & Wilson c. 2007; Hawkes 1999, p. 14; Roza 2009, p. 12
^ Harding, Johnson & Janes 2002, p. 61
^ Merinis, Legoux & Bouissières 1972; Kugler & Keller 1985, pp. 110, 116, 210–211, 224; Takahashi & Otozai 1986; Zuckerman & Hagen 1989, pp. 21–22 (21); Takahashi, Yano & Baba 1992
^ Russell & Lee 2005, p. 299
^ Eberle1985, pp. 190, 192,
^ Brown et al. 2012, p. 264
^ Wiberg 2001, p. 283
^ Eagleson 1994, p. 95
^ Pimpentel 1971, p. 827
^ Messler & Messler 2011, p. 38
^ Fine 1978, p. 718; Emsley 2011, p. 57
^ Thayer 2010, p. 79
^ Berei K & Vasáros 1985, p. 214
^ Pruszyński et al. 2006, pp. 91, 94
^ Zubieta & Zuckerman 2009, p. 260: ‘The compounds AsSn and SbSn, which are classified as alloys of two B subgroup metals, exhibit superconducting properties with a transition temperature of about 4 K.’; Schwartz 2010, p. 32: ‘The metals include the alkali and alkaline earths, beryllium, magnesium, copper, silver, gold and the transition metals. These metals exhibit those characteristics generally associated with the metallic state. The B subgroups comprise the remaining metallic elements. These elements exhibit complex structures and significant departures from typically metallic properties. Aluminum, although considered under the B subgroup metals, is somewhat anomalous as it exhibits many characteristics of a true metal.’
^ Greenwood & Earnshaw 1998, p. 548
^ Phillips & Williams 1965, pp. 4‒5; Steele 1966, p. 66
^ Phillips & Williams 1965, p. 33
^ Wiberg, Holleman & Wiberg 2001, pp. 1253, 1268
^ Steele 1966, p. 67
^ Harrington 1946, pp. 143, 146-147
^ Mingos 1998, pp. 18–19
^ Parish 1977, pp. 201–202
^ Parish 1977, pp. 178
^ Rayner-Canham & Overton 2006, p. 29‒30
^ Pauling 1988, p. 173
^ Vernon 2020, p. 218
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a b Rayner-Canham 2006, pp. 212 − 215
^ Russell & Lee 2005, p. 419
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^ Abrikosov 1988, p. 31
^ Cremer 1965, p. 514
^ Gray 2009, p. 9
^ Taylor et al. 2007, p. 148
^ Oxford English Dictionary 1989, ‘other’
^ Roget’s 21st Century Thesaurus
^ Gray 2010
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^ Slater 1939, p. 444‒445
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^ Joshua 1991, p. 45
^ Farrell & Van Sicien 2007, p. 1442
^ Hill & Holman 2000, p. 40
^ Reid 2011, p. 143
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^ Jezequel & Thomas1997
^ Savitsky 1961, p. 107
^ Hindman 1968, p. 434: ‘The high values obtained for the [electrical] resistivity indicate that the metallic properties of neptunium are closer to the semimetals than the true metals. This is also true for other metals in the actinide series.’; Dunlap et al. 1970, pp. 44, 46: ‘…α-Np is a semimetal, in which covalency effects are believed to also be of importance…For a semimetal having strong covalent bonding, like α-Np…’
^ Strathern 2000, p. 239
^ Roscoe & Schormlemmer 1894, p. 4
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Further reading[edit]
Lowrie RS & Campbell-Ferguson HJ 1971, Inorganic and physical chemistry, 2nd ed., chapter 25: The B-metals, Pergamon Press, Oxford, pp. 306–318
Parish RV 1977, The metallic elements, chapter 9: The p-block metals, Longman, London, pp. 178–199
Phillips CSG & Williams RJP 1966, Inorganic chemistry, vol. 2: Metals, Clarendon Press, Oxford, pp. 459–537
Steele D 1966, The chemistry of the metallic elements, chapter 7: The later B-subgroup metals, Pergamon Press, Oxford, pp. 65–83
hide
vte
Periodic table
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18
1
H
He
2
Li
Be
B
C
N
O
F
Ne
3
Na
Mg
Al
Si
P
S
Cl
Ar
4
K
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
I
Xe
6
Cs
Ba
La
Ce
Pr
Nd
Pm
Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
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
s-block f-block d-block p-block