Editing Group 10 element

{{Short description|Group of chemical elements}}
{{Redirect|Group 10|the rugby league competition|Group 10 Rugby League}}
{{More citations needed|date=December 2009}}
{{Infobox periodic table group
| title       = Group&nbsp;10 {{nowrap|in the periodic table}}
| group number= 10
| trivial name=
| by element  = nickel group
| CAS         = part of VIIIB
| old IUPAC   = part of VIII
| mark        = Ni,Pd,Pt,Ds
| left        = [[Group 9 element|group 9]]
| right       = [[Group 11 element|group 11]]}}
{| class="floatright"
! colspan=2 style="text-align:left;" | ↓&nbsp;<small>[[Period (periodic table)|Period]]</small>
|-
! [[Period 4 element|4]]
| {{element cell image|28|Nickel|Ni| |Solid|Transition metal|Primordial|image=Nickel_electrolytic_and_1cm3_cube.jpg|image caption=A piece of nickel, about 3 cm in size}}
|-
! [[Period 5 element|5]]
| {{element cell image|46|Palladium|Pd| |Solid|Transition metal|Primordial|image=Palladium.jpg|image caption=Palladium crystal}}
|-
! [[Period 6 element|6]]
| {{element cell image|78|Platinum|Pt| |Solid|Transition metal|Primordial|image=Platinum-nugget.jpg|image caption=Platinum nugget}}
|-
! [[Period 7 element|7]]
| {{element cell image|110|Darmstadtium|Ds| |Unknown phase|Unknown chemical properties|Synthetic|legend=unknown chemical properties}}
|-
| colspan="2"|
----
''Legend''
{| style="text-align:center; border:0; margin: 0 auto"
|-
| style="border:{{element color|Primordial}}; background:{{Element color|table mark}}; padding:0 2px;" | [[primordial element]]
|-
| style="border:{{element color|Synthetic}}; background:{{Element color|table mark}}; padding:0 2px;" | [[synthetic element]]
|}
|}

'''Group 10''', numbered by current [[IUPAC]] style, is the [[periodic table group|group]] of [[chemical element]]s in the [[periodic table]] that consists of [[nickel]] (Ni), [[palladium]] (Pd), [[platinum]] (Pt), and [[darmstadtium]] (Ds). All are [[d-block]] [[transition metal]]s. All known [[isotopes]] of darmstadtium are radioactive with short half-lives, and are not known to occur in nature; only minute quantities have been synthesized in laboratories.

==Characteristics==

=== Chemical properties ===
{| class="wikitable" style="white-space:nowrap;"
|-
!''[[Atomic number|Z]]'' !! [[Chemical element|Element]] !! Electrons per [[Electron shell|shell]]
![[Electron configuration|Electronic configuration]]
|-
| 28 || nickel || 2, 8, 16, 2
|{{Mono|[Ar] &nbsp;&nbsp;<sup>&nbsp;&nbsp;</sup> 3d<sup>8</sup> 4s<sup>2</sup>}}
|-
| 46 || palladium || 2, 8, 18, 18
|{{Mono|[Kr] &nbsp;&nbsp;<sup>&nbsp;&nbsp;</sup> 4d<sup>10</sup>}}
|-
| 78 || platinum || 2, 8, 18, 32, 17, 1
|{{Mono|[Xe] 4f<sup>14</sup> 5d<sup>9</sup> 6s<sup>1</sup>}}
|-
| 110 || darmstadtium || 2, 8, 18, 32, 32, 16, 2<br/>(predicted)
|{{Mono|[Rn] 5f<sup>14</sup> 6d<sup>8</sup> 7s<sup>2</sup>}}<br/>(predicted)<ref>{{Citation |last1=Hoffman |first1=Darleane C. |title=Transactinide Elements and Future Elements |url=http://dx.doi.org/10.1007/1-4020-3598-5_14 |work=The Chemistry of the Actinide and Transactinide Elements |pages=1652–1752 |place=Dordrecht |publisher=Springer Netherlands |isbn=978-1-4020-3555-5 |access-date=2022-10-09 |last2=Lee |first2=Diana M. |last3=Pershina |first3=Valeria|year=2006 |doi=10.1007/1-4020-3598-5_14 |url-access=subscription }}</ref>
|}
The ground state electronic configurations of palladium and platinum are exceptions to [[Aufbau principle|Madelung's rule]]. According to Madelung's rule, the electronic configuration of palladium and platinum are expected to be [Kr] 5s<sup>2</sup> 4d<sup>8</sup> and [Xe] 4f<sup>14</sup> 5d<sup>8</sup> 6s<sup>2</sup> respectively. However, the 5s orbital of palladium is empty, and the 6s orbital of platinum is only partially filled. The relativistic stabilization of the 7s orbital is the explanation to the predicted electron configuration of darmstadtium, which, unusually for this group, conforms to that predicted by the [[Aufbau principle]].{{Citation needed|date=November 2022}} In general, the ground state electronic configurations of heavier atoms and transition metals are more difficult to predict.

Group 10 elements are observed in [[oxidation state]]s of +1 to +4.<ref>{{Cite book |last=Lee |first=John David |title=Concise inorganic chemistry |date=2002 |publisher=Blackwell Science |isbn=0-632-05293-7 |edition=5th |pages=803–815 |oclc=}}</ref> The +2 oxidation state is common for nickel and palladium, while +2 and +4 are common for platinum. Oxidation states of −2 and −1 have also been observed for nickel<ref>{{Cite journal |last1=Maier |first1=Thomas M. |last2=Sandl |first2=Sebastian |last3=Melzl |first3=Peter |last4=Zweck |first4=Josef |last5=Jacobi von Wangelin |first5=Axel |last6=Wolf |first6=Robert |date=2020-05-15 |title=Heterogeneous Olefin Hydrogenation Enabled by a Highly-Reduced Nickel(−II) Catalyst Precursor |journal=Chemistry – A European Journal |language=en |volume=26 |issue=28 |pages=6113–6117 |doi=10.1002/chem.201905537 |issn=0947-6539 |pmc=7318650 |pmid=32034810}}</ref><ref>{{Cite journal |last1=Vollmer |first1=Matthew V. |last2=Xie |first2=Jing |last3=Cammarota |first3=Ryan C. |last4=Young |first4=Victor G. |last5=Bill |first5=Eckhard |last6=Gagliardi |first6=Laura |last7=Lu |first7=Connie C. |date=2018-06-25 |title=Formal Nickelate(−I) Complexes Supported by Group 13 Ions |url=https://onlinelibrary.wiley.com/doi/10.1002/ange.201803356 |journal=Angewandte Chemie |language=en |volume=130 |issue=26 |pages=7941–7945 |doi=10.1002/ange.201803356 |bibcode=2018AngCh.130.7941V |s2cid=243890546 |issn=0044-8249|url-access=subscription }}</ref> and platinum,<ref>{{Cite journal |last1=Karpov |first1=Andrey |last2=Konuma |first2=Mitsuharu |last3=Jansen |first3=Martin |date=2006 |title=An experimental proof for negative oxidation states of platinum: ESCA-measurements on barium platinides |url=http://xlink.rsc.org/?DOI=b514631c |journal=Chemical Communications |language=en |issue=8 |pages=838–840 |doi=10.1039/b514631c |pmid=16479284 |issn=1359-7345|url-access=subscription }}</ref> and an oxidation state of +5 has been observed for palladium<ref>{{Cite journal |last1=Shimada |first1=Shigeru |last2=Li |first2=Yong-Hua |last3=Choe |first3=Yoong-Kee |last4=Tanaka |first4=Masato |last5=Bao |first5=Ming |last6=Uchimaru |first6=Tadafumi |date=2007-05-08 |title=Multinuclear palladium compounds containing palladium centers ligated by five silicon atoms |journal=Proceedings of the National Academy of Sciences |language=en |volume=104 |issue=19 |pages=7758–7763 |doi=10.1073/pnas.0700450104 |issn=0027-8424 |pmc=1876520 |pmid=17470819|doi-access=free |bibcode=2007PNAS..104.7758S }}</ref> and platinum.<ref>{{Cite journal |last1=Mueller |first1=B. G. |last2=Serafin |first2=M. |date=2010-08-21 |title=ChemInform Abstract: Single-Crystal Investigations on PtF4 and PtF5. |url=https://onlinelibrary.wiley.com/doi/10.1002/chin.199245006 |journal=ChemInform |language=en |volume=23 |issue=45 |pages=no |doi=10.1002/chin.199245006|url-access=subscription }}</ref> Platinum has also been observed in the oxidation states −3<ref>{{Cite journal |last1=Köhler |first1=Jürgen |last2=Whangbo |first2=Myung-Hwan |date=2008-04-01 |title=Late transition metal anions acting as p-metal elements |url=https://www.sciencedirect.com/science/article/pii/S1293255807003883 |journal=Solid State Sciences |series=Frontiers in Solid State Chemistry |language=en |volume=10 |issue=4 |pages=444–449 |doi=10.1016/j.solidstatesciences.2007.12.001 |bibcode=2008SSSci..10..444K |issn=1293-2558|url-access=subscription }}</ref> and +6.<ref>{{Cite journal |last1=Drews |first1=Thomas |last2=Supeł |first2=Joanna |last3=Hagenbach |first3=Adelheid |last4=Seppelt |first4=Konrad |date=2006-05-01 |title=Solid State Molecular Structures of Transition Metal Hexafluorides |url=https://pubs.acs.org/doi/10.1021/ic052029f |journal=Inorganic Chemistry |language=en |volume=45 |issue=9 |pages=3782–3788 |doi=10.1021/ic052029f |pmid=16634614 |issn=0020-1669|url-access=subscription }}</ref> Theory suggests that platinum may produce a +10 oxidation state under specific conditions, but this remains to be shown empirically.<ref name=":6">{{cite book |last=Rosenberg |first=Samuel J. |url=http://handle.dtic.mil/100.2/ADA381960 |title=Nickel and Its Alloys |date=1968 |publisher=National Bureau of Standards |archive-url=https://web.archive.org/web/20120523193126/http://handle.dtic.mil/100.2/ADA381960 |archive-date=May 23, 2012 |url-status=dead}}</ref>

=== Physical properties ===
{| class="wikitable"
|+Physical properties of the group 10 elements<ref name=":0">{{Cite book |url=https://www.worldcat.org/oclc/957751024 |title=CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data. |date=2017 |others=William M. Haynes, David R. Lide, Thomas J. Bruno |isbn=978-1-4987-5429-3 |edition=97th |location=Boca Raton, Florida |oclc=957751024}}</ref>
!Z
!Element
!Physical form
!Molecular weight
!Density (g/cm<sup>3</sup>)
!Melting point (°C)
!Boiling point (°C)
!Heat capacity/C<sub>p</sub>(c)
(J mol<sup>−1</sup> K<sup>−1</sup>)
!Electron affinity (eV)
!Ionization energy (eV)
|-
|28
|nickel
|white metal; cubic
|{{Center|58.693}}
|{{Center|8.90}}
|{{Center|1455}}
|{{Center|2913}}
|{{Center|26.1}}
|{{Center|1.156}}
|{{Center|7.6399}}
|-
|46
|palladium
|silver-white metal; cubic
|{{Center|106.42}}
|{{Center|12.0}}
|{{Center|1554.8}}
|{{Center|2963}}
|{{Center|26.0}}
|{{Center|0.562}}
|{{Center|8.3369}}
|-
|78
|platinum
|silver-gray metal; cubic
|{{Center|195.048}}
|{{Center|21.5}}
|{{Center|1768.2}}
|{{Center|3825}}
|{{Center|25.9}}
|{{Center|2.128}}
|{{Center|8.9588}}
|}
Darmstadtium has not been isolated in pure form, and its properties have not been conclusively observed; only nickel, palladium, and platinum have had their properties experimentally confirmed. Nickel, platinum, and palladium are typically silvery-white transition metals, and can also be readily obtained in powdered form.<ref name=":2">{{Cite book |last1=Greenwood |first1=N. N. |url=https://www.worldcat.org/oclc/48138330 |title=Chemistry of the elements |last2=Earnshaw |first2=A |date=1997 |publisher=Butterworth-Heinemann |isbn=0-585-37339-6 |edition=2nd |location=Boston, Mass. |oclc=48138330}}</ref> They are hard, have a high [[Lustre (mineralogy)|luster]], and are highly [[ductile]]. Group 10 elements are resistant to tarnish ([[oxidation]]) at [[Standard temperature and pressure|STP]], are [[refractory]], and have high melting and boiling points.

==Occurrence and production==
Nickel occurs naturally in ores, and it is the earth's 22nd most abundant element. Two prominent groups of ores from which it can be extracted are [[laterite]]s and [[sulfide ore]]s.<ref>{{cite web |last1=Lancashire |first1=Robert J. |title=Chemistry of Nickel |url=https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Descriptive_Chemistry/Elements_Organized_by_Block/3_d-Block_Elements/Group_10%3A_Transition_Metals/Chemistry_of_Nickel |website=LibreTexts |date=2 October 2013 |access-date=16 January 2022}}</ref>  [[Indonesia]] holds the world's largest nickel reserve, and is also its largest producer.<ref>{{cite web |title=Reserves of nickel worldwide as of 2020, by country (in million metric tons) |url=https://www.statista.com/statistics/273634/nickel-reserves-worldwide-by-country/ |website=Statista |access-date=16 January 2022}}</ref>

== History ==

=== Discoveries of the elements ===

==== Nickel ====
The use of nickel, often mistaken for copper, dates as far back as 3500 BCE. Nickel has been discovered in a dagger dating to 3100 BCE, in Egyptian iron beads, a bronze reamer found in Syria dating to 3500–3100 BCE, as copper-nickel alloys in coins minted in [[Bactria]], in weapons and pots near the Senegal river, and as agricultural tools used by Mexicans in the 1700s.<ref name=":6" /><ref>{{Cite journal |last=Rickard |first=T. A. |date=1941 |title=The Use of Meteoric Iron |url=https://www.jstor.org/stable/2844401 |journal=The Journal of the Royal Anthropological Institute of Great Britain and Ireland |volume=71 |issue=1/2 |pages=55–66 |doi=10.2307/2844401 |jstor=2844401 |issn=0307-3114|url-access=subscription }}</ref> There is evidence to suggest that the use of nickel in antiquity came from meteoric iron, such as in the Sumerian name for iron ''an-bar'' ("fire from heaven") or in Hittite texts that describe iron's heavenly origins. Nickel was not formally named as an element until A. F. Cronstedt isolated the impure metal from "kupfernickel" (Old Nick's copper) in 1751.'''<ref name=":0"/>''' In 1804, J. B. Richter determined the physical properties of nickel using a purer sample, describing the metal as ductile and strong with a high melting point. The strength of nickel-steel alloys were described in 1889 and since then, nickel steels saw extensive use first for military applications and then in the development of corrosion- and heat-resistant alloys during the 20th century.

==== Palladium ====
Palladium was isolated by [[William Hyde Wollaston]] in 1803 while he was working on refining platinum metals.<ref name=":4"/> Palladium was in a residue left behind after platinum was precipitated out of a solution of [[hydrochloric acid]] and nitric acid as (NH<sub>4</sub>)PtCl<sub>6</sub>.<ref name=":2"/> Wollaston named it after the recently discovered asteroid [[2 Pallas]] and anonymously sold small samples of the metal to a shop, which advertised it as a "new noble metal" called "Palladium, or New Silver".<ref>{{Cite journal |last=Usselman |first=Melvyn C. |date=1978-11-01 |title=The Wollaston/Chenevix controversy over the elemental nature of palladium: A curious episode in the history of chemistry |url=https://doi.org/10.1080/00033797800200431 |journal=Annals of Science |volume=35 |issue=6 |pages=551–579 |doi=10.1080/00033797800200431 |issn=0003-3790|url-access=subscription }}</ref> This raised doubts about its purity, source, and the identity of its discoverer, causing controversy. He eventually identified himself and read his paper on the discovery of palladium to the Royal Society in 1805.<ref>{{Cite journal |last=Wollaston |first=William Hyde |date=1805-01-01 |title=XXII. On the discovery of palladium; with observations on other substances found with plantina |journal=Philosophical Transactions of the Royal Society of London |volume=95 |pages=316–330 |doi=10.1098/rstl.1805.0024|s2cid=97424917 |doi-access=free }}</ref>

==== Platinum ====
Prior to its formal discovery, platinum was used in jewelry by native Ecuadorians of the province of Esmeraldas.<ref name=":1">{{Cite journal |last=Chaston |first=J. C. |date=1980 |title=The Powder Metallurgy of Platinum |url=https://technology.matthey.com/article/24/2/70-79/ |journal=Platinum Metals Review |volume=24 |issue=2 |pages=70–79 |doi=10.1595/003214080X2427079 |via=Johnson Matthey Technology Review|url-access=subscription }}</ref> The metal was found in small grains mixed with gold in river deposits, which the workers sintered with gold to form small trinkets such as rings. The first published report of platinum was written by [[Antonio de Ulloa]], a Spanish mathematician, astronomer, and naval officer who observed "platina" (little silver) in the gold mines of Ecuador during a French expedition in 1736.<ref>{{Cite journal |last=Hunt |first=L. B. |date=1980 |title=Swedish Contributions to the Discovery of Platinum |url=https://technology.matthey.com/article/24/1/31-39/ |journal=Platinum Metals Review |volume=24 |issue=1 |pages=31–39 |doi=10.1595/003214080X2413139 |via=Johnson Matthey Technology Review|url-access=subscription }}</ref> Miners found the "platina" difficult to separate from gold, leading to the abandonment of those mines. [[Charles Wood (ironmaster)]] brought samples of the metal to England in 1741 and investigated its properties, observing its high melting point and its presence as small white grains in black metallic sand. Interest in the metal grew after Wood's findings were reported to the Royal Society. [[Henrik Teofilus Scheffer]], a Swedish scientist, referred to the precious metal as "white gold" and the "seventh metal" in 1751, reporting its high durability, high density, and that it melted easily when mixed with copper or arsenic. Both [[Pierre-François Chabaneau]] (during the 1780s) and William Hyde Wollaston (during the 1800s) developed a powder metallurgy technique to produce malleable platinum, but kept their process a secret.<ref name=":1" /> However, their platinum ingots were brittle and tended to crack easily, likely due to impurities. In the 1800s, furnaces capable of sustaining high temperatures were invented, which eventually replaced powder metallurgy and introduced melted platinum to the market.

==Applications==
The group 10 metals share several uses.  These include:
* Decorative purposes, in the form of [[jewelry]] and [[electroplating]].
* [[Catalysis|Catalysts]] in a variety of [[chemical reaction]]s.
* Metal [[alloys]].
* Electrical components, due to their predictable changes in [[Electrical resistivity and conductivity|electrical resistivity]] with regard to temperature.
* [[Superconductor]]s, as components in alloys with other metals.

==Biological role and toxicity==
Platinum complexes are commonly used in chemotherapy as anticancer drugs due to their antitumor activity. Palladium complexes also show marginal antitumor activity, yet its poor activity is labile compared to platinum complexes.<ref name=":4">{{Cite book |title=Chemistry of the Platinum Group Metals: Recent Developments |date=1991 |publisher=Elsevier |others=F. R. Hartley |isbn=0-444-88189-1 |location=Amsterdam}}</ref>

==See also==
*[[Platinum group]]

==Notes and references==
{{Reflist}}

{{Periodic table (navbox)}}
{{Navbox periodic table}}
{{Group 10 elements}}
{{Authority control}}

{{DEFAULTSORT:Group 10 Element}}
[[Category:Groups (periodic table)]]