|Other metals in the periodic table|
Unknown chemical properties
|Atomic number color shows state at STP:
black=solid, green=Liquid, grey=unknown
In chemistry, other metals is a non-IUPAC approved descriptive phrase for the metallic elements in Groups 13 to 16 of the periodic table. They are physically weak metals that show significant nonmetallic chemistry, consistent with their location between the 'true metals'[n 1] (to their left) and the metalloids (to their right). Among metals they are distinguished by having a combination of relatively low melting points (all less than 950 K) and relatively high electronegativity values (all more than 1.6, revised Pauling).
The descriptive phrase 'other metals' is used here as there is no accepted short-hand term for these metals. Occasionally, some or all of them have instead been referred to as B-subgroup metals, poor metals, or post transition metals; and by at least ten other alternative labels. All of these labels are surveyed later in the main body of this article.
Physically, they are soft (or brittle), mechanically weak metals with melting points lower than those of the transition metals; most also have boiling 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.[n 2]
Chemically, the other metals 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).[n 3]
- 1 Applicable elements
- 2 Properties
- 3 Related groupings
- 4 Notes
- 5 Citations
- 6 References
'Other metals' is not a rigorous IUPAC-approved term. It is a descriptive phrase used here in view of the absence of a widely agreed collective term for the metals in question.[n 5] 'Other' in this sense has the related meanings of, 'Existing besides, or distinct from, that already mentioned'; 'auxiliary', 'ancillary, secondary'. Some or all of these elements have sometimes instead called B-subgroup metals, borderline metals, chemically weak metals, heavy metals (of low melting point), less typical metals, metametals, ordinary metals, p-block metals, peculiar metals, poor metals, post-transition metals,[n 6] semimetals (in the sense of metals with incomplete metallic character)[n 7] or transition metals. These classification groupings are generally found in the same region of the periodic table.
Elements falling into this loose category include aluminium, gallium, indium, thallium, tin, lead, bismuth and polonium. Germanium and antimony are occasionally included as other metals, although they are usually considered to be metalloids.[n 8] Elements 113–117, which are currently allocated the names ununtrium, ununtrium, flerovium, ununpentium, livermorium and ununseptium may be other metals; insufficient quantities of them have been synthesized to allow investigation of their actual physical and chemical properties.[n 9]
On the group 12 transition metals (zinc, cadmium and mercury), Smith observed that, 'Textbook writers have always found difficulty in dealing with these elements.' There is an an abrupt and significant reduction in metallic character from group 11 to group 12.. Their chemistry is that of main group elements. 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.[n 10] 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. The group 12 elements do not satisfy the IUPAC Gold Book definition of a transition metal[n 11] (other than in the case of mercury at 4 K). They are included here only for comparative purposes.
- This section outlines relevant physical and chemical properties of the other metals. For complete profiles, including history, production, specific uses, and biological roles and precautions, see the main article for each element. Abbreviations: MH—Moh's hardness; BCN—bulk coordination number.[n 12]
Zinc is a soft metal (MH 2.5) with poor mechanical properties. It has a crystalline structure (BCN 6+6) that is slightly distorted from the ideal. Many zinc compounds are markedly covalent in character. The oxides of zinc in its preferred oxidation state of +2, namely ZnO and Zn(OH)2, are amphoteric; it forms anionic zincates in strongly basic solutions. Zinc forms Zintl phases such as LiZn, NaZn13 and BaZn13. Highly purified zinc, at room temperature, is ductile. It reacts with moist air to form a thin layer of carbonate that prevents further corrosion.
Cadmium is a soft, ductile metal (MH 2.0) that undergoes substantial deformation, under load, at room temperature. 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. The oxides of cadmium in its preferred oxidation state of +2, namely CdO and CdOH2, are weakly amphoteric; it forms cadmates in strongly basic solutions. Cadmium forms Zintl phases such as LiCd, RbCd13 and CsCd13. 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), the cadmium vapour oxidizes, 'with a reddish-yellow flame, dispersing as an aerosol of potentially lethal CdO particles.' 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.[n 13] Solid mercury (MH 1.5) has a distorted crystalline structure, with mixed metallic-covalent bonding, and a BCN of 6. 'All of the [Group 12] metals, but especially mercury, tend to form covalent rather than ionic compounds.' The oxide of mercury in its preferred oxidation state (HgO; +2) is weakly amphoteric, as is the congener sulfide HgS. It forms anionic thiomercurates (such as Na2HgS2 and BaHgS3) in strongly basic solutions.[n 14] It forms or is a part of Zintl phases such as NaHg and K8In10Hg. Mercury is a relatively inert metal, showing little oxide formation at room temperature.
Aluminium in pure form is a soft metal (MH 3.0) with low mechanical strength. It has a close-packed structure (BCN 12) showing some evidence of partially directional bonding.[n 15] It has a low melting point (just over half that of steel) and a high thermal conductivity. Its strength is halved at 200°C, and for many of its alloys is minimal at 300°C. The latter three properties of aluminium limit its use to situations where fire protection is not required, or necessitate the provision of increased fire protection.[n 16] It bonds covalently in most of its compounds; has an amphoteric oxide; and can form anionic aluminates. Aluminium forms Zintl phases such as LiAl, Ca3Al2Sb6, and SrAl2. A thin protective layer of oxide confers a reasonable degree of corrosion resistance. It is susceptible to attack in low pH (<4) and high (> 8.5) pH conditions,[n 17] a phenomenon that is generally more pronounced in the case of commercial purity aluminium and aluminium alloys. Given many of these properties and its proximity to the dividing line between metals and nonmetals, aluminium is occasionally classified as a metalloid.[n 18] 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; and it has a high electrical conductivity.[n 19] At lower temperatures, aluminium increases its deformation strength (as do most materials) whilst maintaining ductility (as do face-centred cubic metals generally). Chemically, bulk aluminium is a strongly electropositive metal, with a high negative electrode potential.[n 20]
Gallium is a soft, brittle metal (MH 1.5) that melts at only a few degrees above room temperature. It has an unusual crystalline structure featuring mixed metallic-covalent bonding and low symmetry (BCN 7 i.e. 1+2+2+2). It bonds covalently in most of its compounds, has an amphoteric oxide; and can form anionic gallates. Gallium forms Zintl phases such as Li2Ga7, K3Ga13 and YbGa2. It is slowly oxidized in moist air at ambient conditions; a protective film of oxide prevents further corrosion.
Indium is a soft, highly ductile metal (MH 1.0) with a low tensile strength. It has a partially distorted crystalline structure (BCN 4+8) associated with incompletely ionised atoms. The tendency of indium '...to form covalent compounds is one of the more important properties influencing its electrochemical behavior'. 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. Indium forms Zintl phases such as LiIn, Na2In and Rb2In3. Indium does not oxidize in air at ambient conditions.
Thallium is a soft, reactive metal (MH 1.0), so much so that it has no structural uses. 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. 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. It is the only one of the Group 13 elements to react with air at room temperature, slowly forming the amphoteric oxide Tl2O3. It forms anionic thallates such as Tl3TlO3, Na3Tl(OH)6, NaTlO2, and KTlO2, and is present as the Tl– thallide anion in the compound CsTl. Thallium forms Zintl phases, such as Na2Tl, Na2K21Tl19, CsTl and Sr5Tl3H.
Tin is a soft, ductile metal (MH 1.5). It has an irregularly coordinated crystalline structure associated with incompletely ionised atoms. It has a BCN of 4+2. All of the Group 14 elements form compounds in which they are in the +4, predominately covalent, oxidation state; even in the +2 oxidation state tin generally forms covalent bonds. The oxides of tin in its preferred oxidation state of +2, namely SnO and Sn(OH)2, are amphoteric; it forms stannites in strongly basic solutions. 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. It has good corrosion resistance in air on account of forming a thin protective oxide layer. Pure tin has few structural uses but it is used in pewter, as lead-free solder in plumbing and as a hardening agent in alloys of other metals, such as copper, lead, titanium and zinc.
Lead is a soft metal (MH 1.5). 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. It forms a semi-covalent dioxide PbO2; a covalently bonded sulfide PbS; covalently bonded halides; 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. The oxide of lead in its preferred oxidation state (PbO; +2) is amphoteric; it forms anionic plumbates in strongly basic solutions. Lead forms Zintl phases such as CsPb, Sr31Pb20, La5Pb3N and Yb3Pb20. 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.
Bismuth is a slightly radioactive, soft metal (MH 2.5) that is too brittle for any structural use. It has an open-packed crystalline structure (BCN 3+3) with bonding that is intermediate between metallic and covalent. For a metal, it has exceptionally low electrical and thermal conductivity. Most of the ordinary compounds of bismuth are covalent in nature. The oxide, Bi2O3 is predominately basic but will act as a weak acid in warm, very concentrated KOH. It can also be fused with potassium hydroxide in air, resulting in a brown mass of potassium bismuthate. The solution chemistry of bismuth is characterised by the formation of oxyanions; it forns anionic bismuthates in strongly basic solutions. Bismuth forms Zintl phases such as NaBi, Rb7In4Bi6 and Ba11Cd8Bi14. Bailar et al. 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 21]
Polonium is radioactive, soft metal with a hardness similar to lead. It has a simple cublc crystalline structure characterised (as determined by electron density calculations) by partially directional bonding, and a BCN of 6. Such a structure ordinarily results in very low ductility and fracture resistance however polonium has been predicted to be a ductile metal. It forms a covalent hydride; its halides are covalent, volatile compounds, resembling those of tellurium. The oxide of polonium in its preferred oxidation state (PoO2; +4) is predominately basic, but amphoteric if dissolved in concentrated aqueous alkali, or fused with potassium hydroxide in air. The yellow polonate(IV) ion PoO2−
3 is known in aqueous solutions of low Cl‒ concentration and high pH.[n 22] Polonides such as Na2Po, BePo, ZnPo, CdPo and HgPo feature Po2– anions; except for HgPo these are some of the more stable of the polonium compounds.[n 23]
Superficially, the B-subgroup metals are the metals in Groups IB to VIB of the periodic table, corresponding to Groups 11 to 16 using current IUPAC nonmenclature. 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.[n 24]
The B-subgroup metals show nonmetallic properties; this is particularly apparent in moving from group 12 to group 16. Although the group 11 metals have normal close-packed metallic structures they show an overlap in chemical properties. In their +1 compounds (the stable state for silver; less so for copper) they are typical B-subgroup metals. In their +2 and +3 states their chemistry is typical of transition metal compounds.
Parish 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 25]
Chemically weak metals
Rayner-Canham and Overton 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 berylllium, aluminium, zinc, gallium, tin, lead, antimony, bismuth, and polonium.[n 26]
Heavy metals (of low melting point)
Van Wert 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 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.[n 27]
Less typical metals
Habashi groups the elements into eight major categories:  typical metals (alkali metals, alkaline earth metals, and aluminium);  lanthanides (Ce–Lu);  actinides (Th–Lr);  transition metals (Sc, Y, La, Ac, groups 4–10);  less typical metals (groups 11–12, Ga, In, Tl, Sn and Pb);  metalloids (B, Si, Ge, As, Se, Sb, Te, Bi and Po);  covalent nonmetals (H, C, N, O, P, S and the halogens); and  monatomic nonmetals (that is, the noble gases).
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. Sometimes beryllium and gallium are included as metametals despite having low ductility.
Abrikosov 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. Gray identifies as ordinary metals: aluminium, gallium, indium, thallium, element 113, tin, lead, element 114, bismuth, element 115, and element 116. He adds that, 'in reality most of the metals that people think of as ordinary are in fact transition metals...'.
The p-block metals are the metals in groups 13‒15 (or 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.
Slater 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 28] whereas the peculiar metals have structures involving directional bonding. More recently, Joshua observed that the peculiar metals have mixed metallic-covalent bonding.
Farrell and Van Sicien use the term poor metal, for simplicity, 'to denote one with a significant covalent, or directional character.' Hill and Holman 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.'
The term post-transition metal is generally used to describe the category of metallic elements in periods 4–6 of the periodic table, to the right of the transition elements. As this description excludes aluminium, a period 3 metal,[n 29] the post-transition elements thereby form a subset of the other metals. The post-transition metals generally show reduced electropositivity, anionic species formation and a capacity to combine with electropositive metals to give Zintl phases. Compounds of the group 12 metals (zinc, cadmium and mercury) are markedly non-ionic in character, both in structure and properties. Simple cationic chemistry in the group 14 metals, tin and lead, is the exception rather than the norm.
Which elements are counted as post-transition metals depends, in periodic table terms, on where the transition metals are taken to end.[n 30] 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.
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, ytterbium, bismuth, mercury and neptunium. 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' Elementary Treatise on Chemistry, a semimetal was a metallic element with 'very imperfect ductility and malleability' such as zinc, mercury or bismuth.
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.' Cheronis, Parsons and Ronneberg 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 31]
- The true metals comprise Group 11, the transition elements, including the 4f and 5f elements, and the typical members of Groups 1 and 2 (Wells 1985, pp. 1277, 1280).
- Most metals crystallise in close-packed structures with high bulk coordination numbers (8+ to 12, or higher). This is because total metallic bonding energy is optimised in the absence of interatomic gaps and increased when each atom has the greatest possible number of nearest-neighbour atoms. Most metals bordering the nonmetals have more complex structures, with lower bulk coordination numbers (4+ to 6+). This is attributed to the influence of a partial covalent bonding component in the crystal structures of these elements, which dictates fewer nearest neighbours.
- Zintl phases are usually metallic-looking brittle solids, with mixed ionic-covalent bonding, and are typically semiconductors or at least poor metallic conductors hence are sometimes described as semimetals or poor metals.
- 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.' Chemical: The lighter alkaline earths show covalent bonding tendencies (Be predominately; Mg considerably) whereas compounds of the heavier alkaline earths are predominately ionic in nature; the heavier alkaline earths have more stable hydrides and less stable carbides.
- 'Other metals' is also found as a category name for these elements, in the literature. Gray, however, has expressed the view that there should be a better name for these elements than 'other metals'.
- Aluminium sometimes is or is not counted as a post-transition metal.
- Examples include gallium and bismuth.
- Minor, junior or very rare metals. Sazhin, writing on the metallurgy of the rare and minor metals, classifies Hg, Sn, Sb and Bi as 'minor or junior metals', and Ga, In, Tl and Ge as 'very rare metals'. Further metals in this reference are classified as 'light rare metals'—Li, Rb, Cs • Be; rare earths—Sc, Y, lanthanides; 'high-melting rare metals'—Ti, Zr, Hf • V, Cb, Ta • Mo, Nd [sic], Re; and 'radioactive metals'—Ra and the actinides.
- Element 113 is expected to be able to form compounds involving the use of its d-orbital electrons; if this is borne out experimentally, then it would instead be categorized as a transition metal, albeit with significant other metal properties.
- 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.
- 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.
- Moh's hardness values are taken from Samsanov, unless otherwise noted; bulk coordination number values are taken from Darken and Gurry, unless otherwise noted.
- Francium may have a comparably low bonding energy but its melting point of around 27°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.
- Without the use of thermal insulation and detailed structural design attention, 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. 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.
- Aluminium can be attacked, for example, by alkaline detergents (including those used in dishwashers); by wet concrete, and by highly acidic foods such as tomatoes, rhubarb or cabbage. It is not attacked by nitric acid.
- See the list of metalloid lists for references
- Aluminium wire is used in electrical transmisson lines for the distribution of power but, on account of its low breaking strength, is refinforced with a central core of galvanised steel wire.
- 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.
- Which metal has the lowest electrical conductivity is debatable but bismuth is certainly in the lowest cohort; Hoffman refers to bismuth as 'a poor metal, on the verge of being a semiconductor.'
- Bagnall writes that the fusion of polonium dioxide with a potassium chlorate/hydroxide mixture yields a bluish solid which, '...presumably contains some potassium polonate.'
- Bagnall noted that the rare-earth polonides have the greatest thermal stability of any polonium compound.
- Greenwood and Earnshaw 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.'
- Pauling, 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, 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.'
- Aluminium is sometimes referred to as a pre-transition metal, along with the group 1 alkali metals and group 2 alkaline earth metals.
- 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 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 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 is 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.
- In fact, both aluminium (660.32) and germanium (938.25) have melting points greater than 425°C.
- Russell & Lee 2005, p. 5
- Benbow 2008, p. 45; Gupta U 2010, p. 49
- Müller 1992, p. 123
- Evers 2011, p. 58
- Kauzlarich 2005, pp. 6006
- Häussermann 2008, p. 628
- Kauzlarich, Payne & Webb, pp. 45–46, 59
- 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
- Taylor et al. 2007, p. 148; Rankin 2011, p. 388
- Gray 2010
- Oxford English Dictionary 1989, 'other'
- Roget's 21st Century Thesaurus
- Massalski 1986, p. 346: Massalski distinguishes between the noble metals (Cu, Ag and Au), and the 'B subgroup metals', to the right of the noble metals in the periodic table.
- Stott 1956, pp. 99–106; 107; Rayner-Canham & Overton 2006, pp. 29–30: 'There is a subgroup of metals, those closest to the borderline, that exhibit some chemical behaviour that is more typical of the semimetals, particularly formation of anionic species. These nine chemically weak metals are beryllium, aluminium, zinc, gallium, tin, lead, antimony, bismuth, and polonium.'
- Parish 1977, pp. 178–199
- Whitten et al. 2007, p. 868; Cox 2004, p. 185
- Whitten et al. 2007, p. 868
- Cox 2004, p. 185
- Pashaey & Seleznev 1973, p. 565; Gladyshev & Kovaleva 1998, p. 1445; Eason 2007, p. 294
- Jezequel & Thomas 1997, pp. 6620–6
- Sazhin 1961
- 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
- Jensen 2003, p. 952
- Young et al. 1969; Geffner 1969; Jensen 2003
- IUPAC 2005, p. 51
- Crichton 2012, p. 11
- IUPAC 2006–, transition element entry
- Yousif 2007, p. 11; Rosca et al. 2009, pp. 2235–36; Kown et al. 2013
- Samsanov 1968
- Darken & Gurry 1953, pp. 50–53
- Schweitzer 2003, p. 603
- Hutchinson 1964, p. 562
- Greenwood & Earnshaw 1998, p. 1209; Gupta CK 2002, p. 590
- Rayner-Canham & Overton 2006, p. 30
- Kneip 1996, p. xxii
- Russell & Lee 2005, p. 339
- Sequeira 2013, p. 243
- Russell & Lee 2005, p. 349
- Borsari 2005, p. 608
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|Periodic table (Large version)|