Palladium
23319
225573580
2008-07-14T11:09:49Z
Jumbuck
116385
robot Adding: [[ml:പലേഡിയം]]
{{otheruses4|the chemical element}}
{{Elementbox_header | number=46 | symbol=Pd | name=palladium | left=[[rhodium]] | right=[[silver]] | above=[[nickel|Ni]] | below=[[platinum|Pt]] | color1=#ffc0c0 | color2=black }}
{{Elementbox_series | [[transition metal]]s }}
{{Elementbox_groupperiodblock | group=10 | period=5 | block=d }}
{{Elementbox_appearance_img | Pd,46| silvery white metallic }}
{{Elementbox_atomicmass_gpm | [[1 E-25 kg|106.42]][[List of elements by atomic mass|(1)]] }}
{{Elementbox_econfig | [[[krypton|Kr]]] 4d<sup>10</sup> }}
{{Elementbox_epershell | 2, 8, 18, 18, 0 }}
{{Elementbox_section_physicalprop | color1=#ffc0c0 | color2=black }}
{{Elementbox_phase | [[solid]] }}
{{Elementbox_density_gpcm3nrt | 12.023 }}
{{Elementbox_densityliq_gpcm3mp | 10.38 }}
{{Elementbox_meltingpoint | k=1828.05 | c=1554.9 | f=2830.82 }}
{{Elementbox_boilingpoint | k=3236 | c=2963 | f=5365 }}
{{Elementbox_heatfusion_kjpmol | 16.74 }}
{{Elementbox_heatvaporiz_kjpmol | 362 }}
{{Elementbox_heatcapacity_jpmolkat25 | 25.98 }}
{{Elementbox_vaporpressure_katpa | 1721 | 1897 | 2117 | 2395 | 2753 | 3234 | comment= }}
{{Elementbox_section_atomicprop | color1=#ffc0c0 | color2=black }}
{{Elementbox_crystalstruct | cubic face centered }}
{{Elementbox_oxistates | 2, 4<br />(mildly [[base (chemistry)|basic]] oxide) }}
{{Elementbox_electroneg_pauling | 2.20 }}
{{Elementbox_ionizationenergies3 | 804.4 | 1870 | 3177 }}
{{Elementbox_atomicradius_pm | [[1 E-10 m|140]] }}
{{Elementbox_atomicradiuscalc_pm | [[1 E-10 m|169]] }}
{{Elementbox_covalentradius_pm | [[1 E-10 m|131]] }}
{{Elementbox_vanderwaalsrad_pm | [[1 E-10 m|163]] }}
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{{Elementbox_magnetic | no data }}
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{{Elementbox_thermalexpansion_umpmkat25 | 11.8 }}
{{Elementbox_speedofsound_rodmpsat20 | 3070 }}
{{Elementbox_youngsmodulus_gpa | 121 }}
{{Elementbox_shearmodulus_gpa | 44 }}
{{Elementbox_bulkmodulus_gpa | 180 }}
{{Elementbox_poissonratio | 0.39 }}
{{Elementbox_mohshardness | 4.75 }}
{{Elementbox_vickershardness_mpa | 461 }}
{{Elementbox_brinellhardness_mpa | 37.3 }}
{{Elementbox_cas_number | 7440-05-3 }}
{{Elementbox_isotopes_begin | color1=#ffc0c0 | color2=black }}
{{Elementbox_isotopes_decay2 | mn=100 | sym=Pd
| na=[[synthetic radioisotope|syn]] | hl=[[1 E5 s|3.63 d]]
| dm1=[[Electron capture|ε]] | de1=- | pn1=107 | ps1=[[rhodium|Rh]]
| dm2=[[gamma ray|γ]] | de2=0.084, 0.074,<br /> 0.126 | pn2= | ps2=- }}
{{Elementbox_isotopes_stable | mn=102 | sym=Pd | na=1.02% | n=56 }}
{{Elementbox_isotopes_decay | mn=103 | sym=Pd
| na=[[synthetic radioisotope|syn]] | hl=[[1 E6 s|16.991 d]]
| dm=[[Electron capture|ε]] | de=- | pn=103 | ps=[[rhodium|Rh]] }}
{{Elementbox_isotopes_stable | mn=104 | sym=Pd | na=11.14% | n=58 }}
{{Elementbox_isotopes_stable | mn=105 | sym=Pd | na=22.33% | n=59 }}
{{Elementbox_isotopes_stable | mn=106 | sym=Pd | na=27.33% | n=60 }}
{{Elementbox_isotopes_decay | mn=107 | sym=Pd
| na=[[synthetic radioisotope|syn]] | hl=[[1 E14 s|6.5×10<sup>6</sup> y]]
| dm=[[beta emission|β<sup>-</sup>]] | de=0.033 | pn=107 | ps=[[silver|Ag]] }}
{{Elementbox_isotopes_stable | mn=108 | sym=Pd | na=26.46% | n=62 }}
{{Elementbox_isotopes_stable | mn=110 | sym=Pd | na=11.72% | n=64 }}
{{Elementbox_isotopes_end}}
{{Elementbox_footer | color1=#ffc0c0 | color2=black }}
'''Palladium''' (pronounced \pe-‘lä-dē-em\) is a rare and lustrous silvery-white metal that was discovered in 1803 by [[William Hyde Wollaston]], who named it palladium after the [[2_Pallas|asteroid Pallas]], which in turn, was named after the [[epithet]] of the [[Greek mythology|Greek]] goddess [[Athena]], acquired by her when she slew the [[Gigantes|giant]] [[Pallas_%28Giant%29|Pallas]]. The symbol for palladium is '''Pd''', and its [[atomic number]] is 46.
Palladium, along with [[platinum]], [[rhodium]], [[ruthenium]], [[iridium]] and [[osmium]] form a group of elements referred to as the [[platinum group metals]] (PGMs). PGMs share similar chemical properties, but palladium is unique in that it has the lowest melting point and is the least dense of these precious metals. Incredibly, when palladium is at room temperature and atmospheric pressure, it can absorb up to 900 times its own volume of [[hydrogen]], which makes palladium an efficient and safe storage medium for hydrogen and hydrogen isotopes. Palladium is also tarnish resistant, electrically stable and resistant to chemical erosion as well as intense heat.
The unique properties of palladium and other PGMs account for their widespread use. One in four goods manufactured today either contain PGMs or had PGMs play a key role during their manufacturing process. Over half of the supply of palladium and its sister metal [[platinum]] goes into [[catalytic converters]], which convert up to 90% of harmful gases from auto exhaust ([[hydrocarbons]], [[carbon monoxide]] and [[nitrogen oxide]]) into less harmful substances ([[nitrogen]], [[carbon dioxide]] and water vapor). Palladium’s precious metal qualities and appearance generate significant consumption in the luxury [[jewelry]] market. Palladium is found in many electronics including [[computers]], [[mobile phones]], [[multi-layer ceramic capacitors]], [[component plating]], low voltage electrical contacts, and SED/OLED/LCD [[televisions]]. Palladium is also used in [[dentistry]], [[medicine]], hydrogen purification, chemical applications, groundwater treatment, and it plays a key role in the technology used for [[fuel cells]], which combines hydrogen and oxygen to produce electricity, heat and water.
Palladium [[bullion]] has [[ISO currency code]]s of XPD and 964. Palladium is one of only four metals to have such codes, the others being gold, silver and platinum.
[[Ore]] [[deposit]]s of palladium and other PGMs are rare, and the most extensive deposits have been found in the norite belt of the [[Bushveld Igneous Complex]] in the [[Transvaal]] in [[South Africa]], the [[Stillwater igneous complex|Stillwater Complex]] in [[Montana]], [[USA]], the [[Sudbury District]] of [[Ontario]], [[Canada]], and the [[Norilsk Complex]] in [[Russia]]. In addition to [[mining]], [[recycling]] is also a source of palladium, mostly from scrapped catalytic converters. The numerous applications and limited supply sources of palladium result in palladium drawing considerable [[investment]] interest.
== History ==
Palladium was [[discovery of the chemical elements|discovered]] by [[William Hyde Wollaston]] in [[1803]].<ref>{{cite journal | journal = [[Platinum Metals Review]] | url = http://www.platinummetalsreview.com/dynamic/article/view/47-4-175-183 | title = Rhodium and Palladium - Events Surrounding Its Discovery | author = W. P. Griffith | volume = 47 | issue = 4 | date = 2003 | pages = 175–183}}</ref><ref>{{cite journal
| title = On a New Metal, Found in Crude Platina
| author = [[William Hyde Wollaston|W. H. Wollaston]]
| journal = [[Philosophical Transactions of the Royal Society of London]]
| volume = 94
| year = 1804
| pages = 419–430.
| url =
| doi = 10.1098/rstl.1804.0019 }}
</ref> This element was named by Wollaston in 1804 after the asteroid [[2 Pallas|Pallas]], which had been discovered two years earlier.<ref name=lanl/>
Wollaston found palladium in crude platinum ore from [[South America]] by dissolving the ore in [[aqua regia]], neutralizing the solution with [[sodium hydroxide]], and precipitating platinum as [[ammonium chloroplatinate]] with [[ammonium chloride]]. He added [[mercuric cyanide]] to form the compound [[palladium cyanide]], which was heated to extract palladium metal.
[[Palladium chloride]] was at one time prescribed as a [[tuberculosis]] treatment at the rate of 0.065g per day (approximately one milligram per kilogram of body weight). This treatment did have many negative [[Adverse effect (medicine)|side-effects]], and was later replaced by more effective drugs.
Palladium's affinity for hydrogen led it to play an essential role in the [[Fleischmann-Pons experiment]] in 1989, also known as [[cold fusion]].
In the run up to [[2000]], Russian supply of palladium to global market was repeatedly delayed and disrupted<ref>{{cite web | publisher = [[The London Bullion Market Association]] | work = The LBMA Precious Metals Conference 2003 | title = Russian PGM Stocks | author = Alan Williamson | url = http://www.lbma.org.uk/conf2003/5d.williamson%20LBMAConf2003.pdf}}</ref> because the export quota was not granted on time, due to political reasons. The ensuing market panic buying drove the palladium price to an all-time high of $1100 per ounce, reached in January, 2001.<ref>{{cite web |url=http://www.kitco.com/charts/historicalpalladium.html |title=Historical Palladium Charts and Data |publisher=Kitco |accessdate=2007-08-09}}</ref> During the time period, the [[Ford Motor Company]], fearing auto vehicle production disruption due to a possible palladium shortage, stockpiled large amounts of the metal, purchased near the price high. As prices subsequently fell in early [[2001]], Ford lost nearly $1 billion [[United States dollar|U.S. dollars]].
World demand for palladium increased from 100 tons in 1990 to nearly 300 tons in 2000. The global production from mines was 222 metric tons in 2006 according to USGS data.<ref>{{cite web | publisher = [[United States Geological Survey]] | date = January 2007 | title = Platinum-Group Metals | work = Mineral Commodity Summaries | url = http://minerals.usgs.gov/minerals/pubs/commodity/platinum/platimcs07.pdf}}</ref> Most palladium is used for [[catalytic converter]]s in the automobile industry.<ref name=Kielhorn>{{cite journal
| title = Palladium – A review of exposure and effects to human health
| author = J. Kielhorn, C. Melber, D. Keller, I. Mangelsdorf
| journal = International Journal of Hygiene and Environmental Health
| volume = 205
| issue = 6
| year= 2002
| doi = 10.1078/1438-4639-00180 | pages = 417
}}</ref>
== Occurrence ==
[[Image:2005palladium (mined).PNG|thumb|left|Palladium output in 2005]]
In 2005, Russia was the top producer of palladium, with at least 50% world share, followed by South Africa, USA and Canada, reports the [[British Geological Survey]].
Palladium may be found as a free metal alloyed with gold and other platinum group metals in [[placer mining|placer]] deposits of the [[Ural Mountains]], [[Australia]], [[Ethiopia]], [[South America|South]] and [[North America]]. It is commercially produced from [[nickel]]-[[copper]] deposits found in [[South Africa]], [[Ontario]], and [[Siberia]]; the huge volume of ore processed makes this extraction profitable despite the low proportion of palladium in these ores. The world's largest single producer of palladium is [[MMC Norilsk Nickel]] produced from the [[Norilsk|Norilsk–Talnakh]] nickel deposits. The [[Merensky Reef]] of the [[Bushveld Igneous Complex]] of South Africa contains significant palladium in addition to other [[platinum group]] elements. The [[Stillwater igneous complex]] of [[Montana]] also contains mineable palladium.
Palladium is also produced in [[nuclear fission]] reactors and can be extracted from spent nuclear fuel, see [[Synthesis of noble metals]], though the quantity produced is insignificant.
Palladium is found in the rare minerals [[cooperite]] and [[polarite]].
== Characteristics ==
[[Image:Palladium 1.jpg|left|thumb|75px|Palladium.]]
Palladium is a soft silver-white metal that resembles [[platinum]]. It is the least dense and has the lowest [[melting point]] of the [[platinum group]] metals. It is soft and ductile when [[Annealing (metallurgy)|annealed]] and greatly increases its strength and hardness when it is cold-worked. Palladium dissolves slowly in [[sulfuric acid|sulfuric]], [[nitric acid|nitric]], and [[hydrochloric acid]].<ref name=lanl>{{cite web | publisher = [[Los Alamos National Laboratory]] | url = http://periodic.lanl.gov/elements/46.html | title = Palladium | accessdate = 2007-02-05}}</ref> This metal also does not react with [[oxygen]] at normal temperatures (and thus does not tarnish in [[Earth's atmosphere|air]]). Palladium heated to 800°C will produce a layer of palladium(II) oxide (PdO). It lightly tarnishes in moist atmosphere containing sulfur.
This metal has the uncommon ability to [[absorption (chemistry)|absorb]] up to 900 times its own volume of [[hydrogen]] at room temperatures. It is thought that this possibly forms [[palladium hydride]] (PdH<sub>2</sub>) but it is not yet clear if this is a true [[chemical compound]].<ref name=lanl/>
When palladium has absorbed large amounts of hydrogen, it will expand slightly in size.<ref name=Gray>{{cite web
| last = Gray
| first = Theodore
| title = 46 Palladium
| publisher = Element Displays
| url = http://www.theodoregray.com/periodictabledisplay/Elements/046/index.s9.html
| accessdate = 2007-10-14}}</ref>
Common [[oxidation state]]s of palladium are 0,+1, +2 and +4. Although originally +3 was thought of as one of the fundamental oxidation states of palladium, there is no evidence for palladium occurring in the +3 oxidation state; this has been investigated via [[X-ray diffraction]] for a number of compounds, indicating a [[dimer]] of palladium(II) and palladium(IV) instead. Recently, compounds with an oxidation state of +6 were synthesised.
=== Isotopes ===
{{main|isotopes of palladium}}
Naturally-occurring palladium is composed of six [[isotope]]s. The most stable [[radioisotope]]s are [[Pd-107|<sup>107</sup>Pd]] with a [[half-life]] of 6.5 million years, [[Pd-103|<sup>103</sup>Pd]] with a half-life of 17 days, and <sup>100</sup>Pd with a half-life of 3.63 days. Eighteen other radioisotopes have been characterized with [[atomic weight]]s ranging from 92.936 [[atomic mass unit|u]] (<sup>93</sup>Pd) to 119.924 u (<sup>120</sup>Pd). Most of these have half-lives that are less than a half-hour, except <sup>101</sup>Pd (half-life: 8.47 hours), <sup>109</sup>Pd (half-life: 13.7 hours), and <sup>112</sup>Pd (half-life: 21 hours).
The primary [[decay mode]] before the most abundant stable isotope, <sup>106</sup>Pd, is [[electron capture]] and the primary mode after is [[beta decay]]. The primary [[decay product]] before <sup>106</sup>Pd is [[rhodium]] and the primary product after is [[silver]].
[[Radiogenic]] <sup>107</sup>Ag is a decay product of <sup>107</sup>Pd and was first discovered in the [[Santa Clara, California]] meteorite of [[1978]].<ref>{{cite journal
| author= W. R. Kelly, G. J. Wasserburg,
| title = Evidence for the existence of <sup>107</sup>Pd in the early solar system
| journal = [[Geophysical Research Letters]]
| year = 1978
| volume = 5
| issue =
| pages = 1079–1082
| doi = 10.1098/rsta.2001.0893}}</ref> The discoverers suggest that the coalescence and differentiation of iron-cored small planets may have occurred 10 million years after a [[nucleosynthetic]] event. <sup>107</sup>Pd versus Ag correlations observed in bodies, which have clearly been melted since accretion of the [[solar system]], must reflect the presence of short-lived nuclides in the early solar system.<ref>{{cite journal
| author= J. H. Chen, G. J. Wasserburg
| title = The isotopic composition of Ag in meteorites and the presence of <sup>107</sup>Pd in protoplanets
| journal = [[Geochimica et Cosmochimica Acta]]
| year = 1990
| volume = 54
| issue = 6
| pages = 1729–1743
| doi = 10.1016/0016-7037(90)90404-9 }}</ref>
== Applications ==
Palladium is used in [[dentistry]],<ref name=unctad/><ref>{{cite journal | journal = [[Platinum Metals Review]] | title = Palladium in Restorative Dentistry: Superior Physical Properties make Palladium an Ideal Dental Metal | author = Roy Rushforth | volume = 48 | issue = 1 | year = 2004 | url = http://www.platinummetalsreview.com/dynamic/article/view/48-1-030-031}}</ref> [[watch]] making, in blood sugar test strips, in aircraft [[spark plug]]s and in the production of [[surgical instrument]]s and [[electrical contact]]s.{{Fact|date=February 2007}} Palladium is also used to make professional [[transverse flute]]s.{{Fact|date=February 2007}}
===Electronics===
The biggest application of palladium in electronics is making the [[multilayer ceramic capacitor]].<ref>{{cite web | url = http://www.ttiinc.com/object/ME_Zogbi_20030203.html | title = Shifting Supply and Demand for Palladium in MLCCs | author = Dennis Zogbi | date = February 03, 2003 | publisher = TTI, Inc.}}</ref> Palladium (and palladium-[[silver]] alloys) are used as electrodes in multi-layer ceramic [[Capacitor (component)|capacitors]].<ref name=unctad/> Palladium (sometimes alloyed with [[nickel]]) is used in connector platings in consumer electronics.
It is also used in plating of electronic components and in soldering materials. The electronic sector consumed 1.07 million troy ounces of palladium in 2006, according to a [[Johnson Matthey]] report.<ref name = matthey>{{cite web | year = 2007 | publisher = [[Johnson Matthey]] | title = Platinum 2007 | url = http://www.platinum.matthey.com/uploaded_files/2007/07_palladium.pdf | author = David Jollie}}</ref>
===Technology===
Hydrogen easily diffuses through heated palladium; thus, it provides a means of purifying the gas.<ref name=lanl/> [[Membrane reactor]]s with Pd membranes are therefore used for the production of [[hydrogen]].
It is a part of the [[palladium-hydrogen electrode]] in electrochemical studies. [[Palladium (II) chloride]] can absorb large amounts of [[carbon monoxide]] gas, and is used in [[carbon monoxide detectors]].
===Catalysis===
When it is finely divided, such as in [[palladium on carbon]], palladium forms a good [[catalyst]] and is used to speed up [[hydrogenation]] and [[dehydrogenation]] reactions, as well as in [[cracking (chemistry)|petroleum cracking]]. A large number of [[carbon-carbon bond]] forming reactions in [[organic chemistry]] (such as the [[Heck reaction|Heck]] and [[Suzuki coupling]]) are facilitated by catalysis with palladium compounds. The largest use of palladium today is in [[catalytic converters]].<ref name=unctad/>
Pd is also a versatile metal for [[homogeneous catalysis]]. It is used in combination with a broad variety of [[ligands]] for highly selective chemical transformations.
===Hydrogen storage===
{{main|palladium hydride}}
'''Palladium hydride''' is metallic palladium that contains a substantial quantity of [[hydrogen]] within its [[crystal lattice]]. At [[room temperature]] and [[Earth's atmosphere|atmospheric]] [[pressure]], palladium can [[absorption (chemistry)|absorb]] up to 935 times its own volume of hydrogen in a reversible process. This property has been investigated because hydrogen storage is of such interest and a better understanding of what happens at the molecular level could give clues to designing improved [[metal hydride]]s. A palladium based store, however, would be prohibitively expensive due to the cost of the metal.<ref name = grochala >{{cite journal | title = Thermal Decomposition of the Non-Interstitial Hydrides for the Storage and Production of Hydrogen | author = W. Grochala, P. P. Edwards | journal = [[Chem. Rev.]] | year = 2004 | volume = 104 | issue = 3 | pages = 1283–1316 | doi = 10.1021/cr030691s}}</ref>
===Jewelry===
[[Image:Palladium Plated Belt Buckle.jpg|right|thumb|150px|A Palladium plated belt buckle.]]
Palladium itself has been used as a precious metal in [[jewelry]] since 1939, as an alternative to [[platinum]] or [[white gold]]. This is due to its naturally white properties, giving it no need for [[rhodium]] plating. It is slightly whiter, much lighter and about 12% harder than platinum. Similar to gold, palladium can be beaten into a thin leaf form as thin as 100 nm (1/250,000 in).<ref name=lanl/> Like platinum, it will develop a hazy [[patina]] over time. Unlike [[platinum]], however, palladium may discolor at high [[soldering]] temperatures, become brittle with repeated heating and cooling, and react with strong acids.{{fact|date=January 2008}}
It can also be used as a substitute for nickel when making white gold. Palladium is one of the three most popular metals used to alloy with gold, making white gold.<ref name=unctad>{{cite web | publisher = [[United Nations Conference on Trade and Development]] | url = http://www.unctad.org/infocomm/anglais/palladium/uses.htm | title = Palladium | accessdate = 2007-02-05}}</ref> ([[Nickel]] and [[silver]] can also be used.) Palladium-gold is a more expensive alloy than nickel-gold, but it's naturally [[hypoallergenic]] and holds its white color better.
When platinum was declared a strategic government resource during [[World War II]], many jewelry bands were made out of palladium. As recently as September 2001,<ref>{{cite web | publisher = [[Johnson Matthey]] | title = Daily Metal Prices: September 2001 | url = http://www.platinum.matthey.com/prices/September2001.php}}</ref> palladium was more expensive than platinum and rarely used in jewelry also due to the technical obstacle of [[casting]]. However the casting problem has been resolved, and its use in jewelry has increased because of a large spike in the price of platinum and a drop in the price of palladium.<ref name=wsj>{{cite news | author = Holmes, E. | title = Palladium, Platinum's Cheaper Sister, Makes a Bid for Love | publisher = [[Wall Street Journal]] (Eastern edition) | date = Feb 13, 2007 | pages = B.1}}</ref>
Prior to 2004, the principal use of palladium in jewelry was as an alloy in the manufacture of white gold jewelry, but, beginning early in 2004 when gold and platinum prices began to rise steeply, Chinese jewelers began fabricating significant volumes of palladium jewelry. Johnson Matthey estimated that in 2004, with the introduction of palladium jewelry in China, demand for palladium for jewelry fabrication was 920,000 ounces, or approximately 14% of the total palladium demand for 2004 - an increase of almost 700,000 ounces from the previous year. This growth continued during 2005, with estimated worldwide jewelry demand for palladium of about 1.4 million ounces, or almost 21% of net palladium supply, again with most of the demand centered in China. The popularity of Palladium jewelry is expected to grow in 2008 as the world's biggest producers embark on a joint marketing effort to promote Palladium jewelry worldwide <ref>{{cite web | publisher = [[Yahoo Finance]] | title = Stillwater Mining Up on Jewelry Venture | url = http://biz.yahoo.com/ap/080311/stillwater_mining_mover.html}}</ref>
===Photography===
{{main|Palladium processing}}
With the [[platinotype]] printing process photographers make fine-art black-and-white prints using platinum or palladium salts. Often used with platinum, palladium provides an alternative to silver.<ref>{{cite journal
| author = Mike Ware
| title = Book Review of : Photography in Platinum and Palladium
| journal = [[Platinum Metals Review]]
| volume = 49
| issue = 4
| pages = 190–195
| year = 2005
| doi = 10.1595/147106705X70291}}
</ref>
===Art===
{{main|Palladium processing}}
Palladium leaf is one of several alternatives to silver leaf used in [[Illuminated manuscript|manuscript illumination]]. The use of silver leaf is problematic due to its predisposition to tarnish. [[Aluminium]] leaf is a very inexpensive alternative, however aluminium is much more difficult to work than gold or silver and results in less than optimal results when employing traditional metal leafing techniques, and so palladium leaf is considered the best substitute despite its considerable cost. Platinum leaf may be used to the same effect as palladium leaf with similar working properties, but it is not as readily available in leaf form commercially.<ref>{{cite book
| author = Margaret Morgan
| title = The Bible of Illuminated Letters
| publisher = Barron's Educational Series
| ISBN-10 = 0764158201
| ISBN-13 = 978-0764158209
| page = 50
| year = 2007}}
</ref><ref>{{cite web | publisher = [[Theodore Gray]] | title = Palladium Leaf | url = http://www.theodoregray.com/PeriodicTable/Samples/046.6/index.s12.html}}</ref>
==See also==
* [[Palladium coin]]
* [[Precious metal]]
* [[Palladium as an investment]]
* [[:Category:Palladium compounds|Palladium compounds]]
* [[Platinum]]
* [[Periodic Table]]
==References==
<div class="references-small">
<references/>
</div>
== External links ==
{{Commons|Palladium}}
{{wiktionary|palladium}}
*[http://www.kitco.com/charts/livepalladium.html Current and Historical Palladium Price]
*[http://www.pse-mendelejew.de/bilder/pd.jpg picture of 999.5 fine Palladium in the element collection from Heinrich Pniok]
{{clear}}
{{compact periodic table}}
{{Jewellery Materials}}
[[Category:Palladium|*]]
[[Category:Chemical elements]]
[[Category:Transition metals]]
[[Category:Precious metals]]
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[[ca:Pal·ladi (element)]]
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