Palladium

This article is about the chemical element. For other uses, see Palladium (disambiguation).

Not to be confused with Platinum.

Palladium is a chemical element with the symbol Pd and atomic number 46. It is a rare and lustrous silvery-white metal discovered in 1803 by the English chemist William Hyde Wollaston. He named it after the asteroid Pallas, which was itself named after the epithet of the Greek goddess Athena, acquired by her when she slew Pallas. Palladium, platinum, rhodium, ruthenium, iridium and osmium form a group of elements referred to as the platinum group metals (PGMs). They have similar chemical properties, but palladium has the lowest melting point and is the least dense of them.

Palladium, ₄₆Pd

Palladium
Pronunciation	/pəˈleɪdiəm/ ​(pə-LAY-dee-əm)
Appearance	silvery white
Standard atomic weight Ar°(Pd)
	106.42±0.01 106.42±0.01 (abridged)^[1]
Palladium in the periodic table
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson Ni ↑ Pd ↓ Pt rhodium ← palladium → silver
Atomic number (Z)	46
Group	group 10
Period	period 5
Block	d-block
Electron configuration	[Kr] 4d^10
Electrons per shell	2, 8, 18, 18
Physical properties
Phase at STP	solid
Melting point	1828.05 K ​(1554.9 °C, ​2830.82 °F)
Boiling point	3236 K ​(2963 °C, ​5365 °F)
Density (near r.t.)	12.023 g/cm^3
when liquid (at m.p.)	10.38 g/cm^3
Heat of fusion	16.74 kJ/mol
Heat of vaporization	358 kJ/mol
Molar heat capacity	25.98 J/(mol·K)
Vapor pressure P (Pa) 1 10 100 1 k 10 k 100 k at T (K) 1721 1897 2117 2395 2753 3234
Atomic properties
Oxidation states	0, +1, +2, +3, +4, +5^[2] (a mildly basic oxide)
Electronegativity	Pauling scale: 2.20
Ionization energies	1st: 804.4 kJ/mol 2nd: 1870 kJ/mol 3rd: 3177 kJ/mol
Atomic radius	empirical: 137 pm
Covalent radius	139±6 pm
Van der Waals radius	163 pm
Spectral lines of palladium
Other properties
Natural occurrence	primordial
Crystal structure	​face-centered cubic (fcc)
Speed of sound thin rod	3070 m/s (at 20 °C)
Thermal expansion	11.8 µm/(m⋅K) (at 25 °C)
Thermal conductivity	71.8 W/(m⋅K)
Electrical resistivity	105.4 nΩ⋅m (at 20 °C)
Magnetic ordering	paramagnetic^[3]
Molar magnetic susceptibility	+567.4×10^−6 cm^3/mol (288 K)^[4]
Young's modulus	121 GPa
Shear modulus	44 GPa
Bulk modulus	180 GPa
Poisson ratio	0.39
Mohs hardness	4.75
Vickers hardness	400–600 MPa
Brinell hardness	320–610 MPa
CAS Number	7440-05-3
History
Naming	after asteroid Pallas, itself named after Pallas Athena
Discovery and first isolation	William Hyde Wollaston (1802)
Isotopes of palladium v e
Main isotopes^[5] Decay abun­dance half-life (t1/2) mode pro­duct ^100Pd synth 3.63 d ε ^100Rh γ – ^102Pd 1.02% stable ^103Pd synth 16.991 d ε ^103Rh ^104Pd 11.1% stable ^105Pd 22.3% stable ^106Pd 27.3% stable ^107Pd trace 6.5×10^6 y β^− ^107Ag ^108Pd 26.5% stable ^110Pd 11.7% stable
Category: Palladium view talk edit | references

More than half the supply of palladium and its congener platinum is used in catalytic converters, which convert as much as 90% of the harmful gases in automobile exhaust (hydrocarbons, carbon monoxide, and nitrogen dioxide) into nontoxic substances (nitrogen, carbon dioxide and water vapor). Palladium is also used in electronics, dentistry, medicine, hydrogen purification, chemical applications, groundwater treatment, and jewelry. Palladium is a key component of fuel cells, in which hydrogen and oxygen react to produce electricity, heat, and water.

Ore deposits of palladium and other PGMs are rare. The most extensive deposits have been found in the norite belt of the Bushveld Igneous Complex covering the Transvaal Basin in South Africa, the Stillwater Complex in Montana, United States; the Sudbury Basin and Thunder Bay District of Ontario, Canada, and the Norilsk Complex in Russia. Recycling is also a source, mostly from scrapped catalytic converters. The numerous applications and limited supply sources result in considerable investment interest.

Characteristics

Palladium belongs to group 10 in the periodic table, but the configuration in the outermost electrons is in accordance with Hund's rule. Electrons that by the Madelung rule would be expected to occupy the 5s instead fill the 4d orbitals, as it is more energetically favorable to have a completely filled 4d¹⁰ shell instead of the 5s² 4d⁸ configuration.^{[clarification needed]}

Z	Element	No. of electrons/shell
28	nickel	2, 8, 16, 2 (or 2, 8, 17, 1)
46	palladium	2, 8, 18, 18, 0
78	platinum	2, 8, 18, 32, 17, 1
110	darmstadtium	2, 8, 18, 32, 32, 16, 2 (predicted)

This 5s⁰ configuration, unique in period 5, makes palladium the heaviest element having only one incomplete electron shell, with all shells above it empty.

Palladium has the appearance of 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 annealed and is greatly increased in strength and hardness when cold-worked. Palladium dissolves slowly in concentrated nitric acid, in hot, concentrated sulfuric acid, and when finely ground, in hydrochloric acid.^[6] It dissolves readily at room temperature in aqua regia.

Palladium does not react with oxygen at standard temperature (and thus does not tarnish in air). Palladium heated to 800 °C will produce a layer of palladium(II) oxide (PdO). It may slowly develop a slight brownish coloration over time, likely due to the formation of a surface layer of its monoxide.

Palladium films with defects produced by alpha particle bombardment at low temperature exhibit superconductivity having T_c=3.2 K.^[7]

Isotopes

Main article: Isotopes of palladium

Naturally occurring palladium is composed of seven isotopes, six of which are stable. The most stable radioisotopes are ¹⁰⁷Pd with a half-life of 6.5 million years (found in nature), ¹⁰³Pd with 17 days, and ¹⁰⁰Pd with 3.63 days. Eighteen other radioisotopes have been characterized with atomic weights ranging from 90.94948(64) u (⁹¹Pd) to 122.93426(64) u (¹²³Pd).^[8] These have half-lives of less than thirty minutes, except ¹⁰¹Pd (half-life: 8.47 hours), ¹⁰⁹Pd (half-life: 13.7 hours), and ¹¹²Pd (half-life: 21 hours).^[9]

For isotopes with atomic mass unit values less than that of the most abundant stable isotope, ¹⁰⁶Pd, the primary decay mode is electron capture with the primary decay product being rhodium. The primary mode of decay for those isotopes of Pd with atomic mass greater than 106 is beta decay with the primary product of this decay being silver.^[9]

Radiogenic ¹⁰⁷Ag is a decay product of ¹⁰⁷Pd and was first discovered in 1978^[10] in the Santa Clara^[11] meteorite of 1976. The discoverers suggest that the coalescence and differentiation of iron-cored small planets may have occurred 10 million years after a nucleosynthetic event. ¹⁰⁷Pd versus Ag correlations observed in bodies, which have been melted since accretion of the Solar System, must reflect the presence of short-lived nuclides in the early Solar System.^{[12] 107}
Pd is also produced as a fission product in spontaneous or induced fission of ²³⁵
U. As it is not very mobile in the environment and has a relatively low decay energy, ¹⁰⁷
Pd is usually considered to be among the less concerning of the long-lived fission products.

Compounds

See also: Category:Palladium compounds

Palladium compounds exist primarily in the 0 and +2 oxidation state. Other less common states are also recognized. Generally the compounds of palladium are more similar to those of platinum than those of any other element.

•  

  Structure of α-PdCl₂

•  

  Structure of β-PdCl₂

Palladium(II)

Palladium(II) chloride is the principal starting material for other palladium compounds. It arises by the reaction of palladium with chlorine. It is used to prepare heterogeneous palladium catalysts such as palladium on barium sulfate, palladium on carbon, and palladium chloride on carbon.^[13] Solutions of PdCl₂ in nitric acid react with acetic acid to give palladium(II) acetate, also a versatile reagent. PdCl₂ reacts with ligands (L) to give square planar complexes of the type PdCl₂L₂. One example of such complexes is the benzonitrile derivative PdX₂(PhCN)₂.^[14][15]

PdCl₂ + 2 L → PdCl₂L₂ (L = PhCN, PPh₃, NH₃, etc)

The complex bis(triphenylphosphine)palladium(II) dichloride is a useful catalyst.^[16]

 

Palladium(II) acetate

 

Platinum-palladium ore from the Stillwater mine in the Beartooth Mountains, Montana, USA

 

Sulfidic serpentintite (platinum-palladium ore) from the Stillwater mine in Montana

Palladium(0)

Palladium forms a range of zerovalent complexes with the formula PdL₄, PdL₃ and PdL₂. For example, reduction of a mixture of PdCl₂(PPh₃)₂ and PPh₃ gives tetrakis(triphenylphosphine)palladium(0):^[17]

2 PdCl₂(PPh₃)₂ + 4 PPh₃ + 5 N₂H₄ → 2 Pd(PPh₃)₄ + N₂ + 4 N₂H₅⁺Cl⁻

Another major palladium(0) complex, tris(dibenzylideneacetone)dipalladium(0) (Pd₂(dba)₃), is prepared by reducing sodium tetrachloropalladate in the presence of dibenzylideneacetone.^[18]

Palladium(0), as well as palladium(II), are catalysts in coupling reactions, as has been recognized by the 2010 Nobel Prize in Chemistry to Richard F. Heck, Ei-ichi Negishi, and Akira Suzuki. Such reactions are widely practiced for the synthesis of fine chemicals. Prominent coupling reactions include the Heck, Suzuki, Sonogashira coupling, Stille reactions, and the Kumada coupling. Palladium(II) acetate, tetrakis(triphenylphosphine)palladium(0) (Pd(PPh₃)₄, and tris(dibenzylideneacetone)dipalladium(0) (Pd₂(dba)₃) serve either as catalysts or precatalysts.^[19]

Other oxidation states

Although Pd(IV) compounds are comparatively rare, one example is sodium hexachloropalladate(IV), Na₂[PdCl₆]. A few compounds of palladium(III) are also known.^[20] Palladium(VI) was claimed in 2002,^[21][22] but subsequently disproven.^[23][24]

Mixed valence palladium complexes exist, e.g. Pd₄(CO)₄(OAc)₄Pd(acac)₂ forms an infinite Pd chain structure, with alternatively interconnected Pd₄(CO)₄(OAc)₄ and Pd(acac)₂ units.^[25]

When alloyed with a more electropositive element, palladium can acquire a negative charge. Such compounds are known as palladides, such as gallium palladide.^[26] Palladides with the stoichiometry RPd₃ exist where R is scandium, yttrium, or any of the lanthanides.^[27]

Occurrence

 

Palladium output in 2005

As overall mine production of palladium reached 210,000 kilograms in 2022, Russia was the top producer with 88,000 kilograms, followed by South Africa, Canada, the U.S., and Zimbabwe.^[28] Russia's company Norilsk Nickel ranks first among the largest palladium producers globally, accounting for 39% of the world's production.^[29]

Palladium can be found as a free metal alloyed with gold and other platinum-group metals in placer deposits of the Ural Mountains, Australia, Ethiopia, North and South America. For the production of palladium, these deposits play only a minor role. The most important commercial sources are nickel-copper deposits found in the Sudbury Basin, Ontario, and the Norilsk–Talnakh deposits in Siberia. The other large deposit is the Merensky Reef platinum group metals deposit within the Bushveld Igneous Complex South Africa. The Stillwater igneous complex of Montana and the Roby zone ore body of the Lac des Îles igneous complex of Ontario are the two other sources of palladium in Canada and the United States.^[30][31] Palladium is found in the rare minerals cooperite^[32] and polarite.^[33] Many more Pd minerals are known, but all of them are very rare.^[34]

Palladium is also produced in nuclear fission reactors and can be extracted from spent nuclear fuel (see synthesis of precious metals), though this source for palladium is not used. None of the existing nuclear reprocessing facilities are equipped to extract palladium from the high-level radioactive waste.^[35] A complication for the recovery of Palladium in spent fuel is the presence of ¹⁰⁷
Pd, a slightly radioactive long-lived fission product. Depending on end use, the radioactivity contributed by the ¹⁰⁷
Pd might make the recovered Palladium unusable without a costly step of isotope separation.

Applications

 

Cross section of a metal-core catalytic converter

 

The Soviet 25-rouble commemorative palladium coin is a rare example of the monetary usage of palladium.

The largest use of palladium today is in catalytic converters.^[36] Palladium is also used in jewelry, dentistry,^[36][37] watch making, blood sugar test strips, aircraft spark plugs, surgical instruments, and electrical contacts.^[38] Palladium is also used to make professional transverse (concert or classical) flutes.^[39] As a commodity, palladium bullion has ISO currency codes of XPD and 964. Palladium is one of only four metals to have such codes, the others being gold, silver and platinum.^[40] Because it adsorbs hydrogen, palladium was a key component of the controversial cold fusion experiments of the late 1980s.^[41]

Catalysis

When it is finely divided, as with palladium on carbon, palladium forms a versatile catalyst; it speeds heterogeneous catalytic processes like hydrogenation, dehydrogenation, and petroleum cracking. Palladium is also essential to the Lindlar catalyst, also called Lindlar's Palladium.^[42] A large number of carbon–carbon bonding reactions in organic chemistry are facilitated by palladium compound catalysts. For example:

• Heck reaction
• Suzuki coupling
• Tsuji-Trost reactions
• Wacker process
• Negishi reaction
• Stille coupling
• Sonogashira coupling

(See palladium compounds and palladium-catalyzed coupling reactions.)

When dispersed on conductive materials, palladium is an excellent electrocatalyst for oxidation of primary alcohols in alkaline media.^[43] Palladium is also a versatile metal for homogeneous catalysis, used in combination with a broad variety of ligands for highly selective chemical transformations.

In 2010 the Nobel Prize in Chemistry was awarded "for palladium-catalyzed cross couplings in organic synthesis" to Richard F. Heck, Ei-ichi Negishi and Akira Suzuki. A 2008 study showed that palladium is an effective catalyst for carbon-fluorine bonds.^[44]

 

Catalytic cycle for Kumada cross coupling reaction, which is widely used in the synthesis of fine chemicals.

Palladium catalysis is primarily employed in organic chemistry and industrial applications, although its use is growing as a tool for synthetic biology; in 2017, effective in vivo catalytic activity of palladium nanoparticles was demonstrated in mammals to treat disease.^[45]

Electronics

The primary application of palladium in electronics is in multi-layer ceramic capacitors^[46] in which palladium (and palladium-silver alloy) is used for electrodes.^[36] Palladium (sometimes alloyed with nickel) is or can be used for component and connector plating in consumer electronics^[47][48] and in soldering materials. The electronic sector consumed 1.07 million troy ounces (33 tonnes) of palladium in 2006, according to a Johnson Matthey report.^[49]

Technology

Hydrogen easily diffuses through heated palladium,^[6] and membrane reactors with Pd membranes are used in the production of high purity hydrogen.^[50] Palladium is used in palladium-hydrogen electrodes in electrochemical studies. Palladium(II) chloride readily catalyzes carbon monoxide gas to carbon dioxide and is useful in carbon monoxide detectors.^[51]

Hydrogen storage

Main article: Palladium hydride

Palladium readily adsorbs hydrogen at room temperatures, forming palladium hydride PdH_x with x less than 1.^[52] While this property is common to many transition metals, palladium has a uniquely high absorption capacity and does not lose its ductility until x approaches 1.^[53] This property has been investigated in designing an efficient and safe hydrogen fuel storage medium, though palladium itself is currently prohibitively expensive for this purpose.^[54] The content of hydrogen in palladium can be linked to magnetic susceptibility, which decreases with the increase of hydrogen and becomes zero for PdH_0.62. At any higher ratio, the solid solution becomes diamagnetic.^[55]

Palladium is also used for hydrogen purification via hydrogen-purification membranes.^{[56]: 183–217 [57]}

Dentistry

Palladium is used in small amounts (about 0.5%) in some alloys of dental amalgam to decrease corrosion and increase the metallic lustre of the final restoration.^[58][59]

Jewelry

Palladium has been used as a precious metal in jewelry since 1939 as an alternative to platinum in the alloys called "white gold", where the naturally white color of palladium does not require rhodium plating. Palladium, being much less dense than platinum, is similar to gold in that it can be beaten into leaf as thin as 100 nm (1⁄250,000 in).^[6] Unlike platinum, palladium may discolor at temperatures above 400 °C (752 °F)^[60] due to oxidation, making it more brittle and thus less suitable for use in jewelry; to prevent this, palladium intended for jewelry is heated under controlled conditions.^{[citation needed]}

Prior to 2004, the principal use of palladium in jewelry was the manufacture of white gold. Palladium is one of the three most popular alloying metals in white gold (nickel and silver can also be used).^[36] Palladium-gold is more expensive than nickel-gold, but seldom causes allergic reactions (though certain cross-allergies with nickel may occur).^[61]

When platinum became a strategic resource during World War II, many jewelry bands were made out of palladium. Palladium was little used in jewelry because of the technical difficulty of casting. With the casting problem resolved^[62] the use of palladium in jewelry increased, originally because platinum increased in price while the price of palladium decreased.^[63] In early 2004, when gold and platinum prices rose steeply, China began fabricating volumes of palladium jewelry, consuming 37 tonnes in 2005. Subsequent changes in the relative price of platinum lowered demand for palladium to 17.4 tonnes in 2009.^[64][65] Demand for palladium as a catalyst has increased the price of palladium to about 50% higher than that of platinum in January 2019.^[66]

In January 2010, hallmarks for palladium were introduced by assay offices in the United Kingdom, and hallmarking became mandatory for all jewelry advertising pure or alloyed palladium. Articles can be marked as 500, 950, or 999 parts of palladium per thousand of the alloy.

Fountain pen nibs made from gold are sometimes plated with palladium when a silver (rather than gold) appearance is desired. Sheaffer has used palladium plating for decades, either as an accent on otherwise gold nibs or covering the gold completely.

Palladium is also used by the luxury brand Hermes as one of the metals plating the hardware on their handbags, most famous of which being Birkin.

Photography

In 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.^[67]

Effects on health

Toxicity

Palladium

Hazards
GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H317
Precautionary statements	P261, P273, P280, P302+P352, P321, P333+P313, P363, P501^[68]
NFPA 704 (fire diamond)	0 0 0

Palladium is a metal with low toxicity as conventionally measured (e.g. LD₅₀). Recent research on the mechanism of palladium toxicity suggests high toxicity if measured on a longer timeframe and at the cellular level in the liver and kidney.^[69] Mitochondria appear to have a key role in palladium toxicity via mitochondrial membrane potential collapse and depletion of the cellular glutathione (GSH) level. Until that recent work, it had been thought that palladium was poorly absorbed by the human body when ingested. Plants such as the water hyacinth are killed by low levels of palladium salts, but most other plants tolerate it, although tests show that, at levels above 0.0003%, growth is affected. High doses of palladium could be poisonous; tests on rodents suggest it may be carcinogenic, though until the recent research cited above, no clear evidence indicated that the element harms humans.^[70]

Precautions

Like other platinum-group metals, bulk Pd is quite inert. Although contact dermatitis has been reported, data on the effects are limited. It has been shown that people with an allergic reaction to palladium also react to nickel, making it advisable to avoid the use of dental alloys containing palladium on those so allergic.^{[71][72][73][74][75]}

Some palladium is emitted with the exhaust gases of cars with catalytic converters. Between 4 and 108 ng/km of palladium particulate is released by such cars, while the total uptake from food is estimated to be less than 2 µg per person a day. The second possible source of palladium is dental restoration, from which the uptake of palladium is estimated to be less than 15 µg per person per day. People working with palladium or its compounds might have a considerably greater uptake. For soluble compounds such as palladium chloride, 99% is eliminated from the body within 3 days.^[71]

The median lethal dose (LD₅₀) of soluble palladium compounds in mice is 200 mg/kg for oral and 5 mg/kg for intravenous administration.^[71]

History

 

William Hyde Wollaston

William Hyde Wollaston noted the discovery of a new noble metal in July 1802 in his lab book and named it palladium in August of the same year. Wollaston purified a quantity of the material and offered it, without naming the discoverer, in a small shop in Soho in April 1803. After harsh criticism from Richard Chenevix, who claimed that palladium was an alloy of platinum and mercury, Wollaston anonymously offered a reward of £20 for 20 grains of synthetic palladium alloy.^[76] Chenevix received the Copley Medal in 1803 after he published his experiments on palladium. Wollaston published the discovery of rhodium in 1804 and mentions some of his work on palladium.^[77][78] He disclosed that he was the discoverer of palladium in a publication in 1805.^[76][79]

It was named by Wollaston in 1802 after the asteroid 2 Pallas, which had been discovered two months earlier.^[6] 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(II) cyanide, which was heated to extract palladium metal.^[77]

Palladium chloride was at one time prescribed as a tuberculosis treatment at the rate of 0.065 g per day (approximately one milligram per kilogram of body weight). This treatment had many negative side-effects, and was later replaced by more effective drugs.^[80]

Most palladium is used for catalytic converters in the automobile industry.^[71] Catalytic converters are targets for thieves because they contain palladium and other rare metals. In the run up to year 2000, the Russian supply of palladium to the global market was repeatedly delayed and disrupted; for political reasons, the export quota was not granted on time.^[81] The ensuing market panic drove the price to an all-time high of $1,340 per troy ounce ($43/g) in January 2001.^[82] Around that time, the Ford Motor Company, fearing that automobile production would be disrupted by a palladium shortage, stockpiled the metal. When prices fell in early 2001, Ford lost nearly US$1 billion.^[83]

World demand for palladium increased from 100 tons in 1990 to nearly 300 tons in 2000. The global production of palladium from mines was 222 tonnes in 2006 according to the United States Geological Survey.^[30] Many were concerned about a steady supply of palladium in the wake of Russia's annexation of Crimea, partly as sanctions could hamper Russian palladium exports; any restrictions on Russian palladium exports could have exacerbated what was already expected to be a large palladium deficit in 2014.^[84] Those concerns pushed palladium prices to their highest level since 2001.^[85] In September 2014 they soared above the $900 per ounce mark. In 2016 however palladium cost around $614 per ounce as Russia managed to maintain stable supplies.^[86] In January 2019 palladium futures climbed past $1,344 per ounce for the first time on record, mainly due to the strong demand from the automotive industry.^[87] Palladium reached $2,024.64 per troy ounce ($65.094/g) on 6 January 2020, passing $2,000 per troy ounce the first time.^[88] The price rose above $3,000 per troy ounce in May 2021 and March 2022.^[89]

Palladium as investment

 

Palladium Prices
US Dollars per troy ounce

Global palladium sales were 8.84 million ounces (250.6 tonnes) in 2017,^[90] of which 86% was used in the manufacturing of automotive catalytic converters, followed by industrial, jewelry, and investment usages.^[91] More than 75% of global platinum and 40% of palladium are mined in South Africa. Russia's mining company, Norilsk Nickel, produces another 44% of palladium, with US and Canada-based mines producing most of the rest.

The price for palladium reached an all-time high of $2,981.40 per ounce on May 3, 2021^[92][93] driven mainly on speculation of the catalytic converter demand from the automobile industry. Palladium is traded in the spot market with the code "XPD". When settled in USD, the code is "XPDUSD". A later surplus of the metal was caused by the Russian government selling stockpiles from the Soviet Era, at a rate of about 1.6 to 2 million ounces (45.4 to 56.7 t) a year. The amount and status of this stockpile are a state secret.

During the Russo-Ukrainian War in March 2022, prices for palladium increased 13%, since the first of March. Russia is the primary supplier to Europe and the country supplies 37% of the global production.^[94]

Palladium producers

• Norilsk Nickel (MCX: GMKN, LSE: MNOD), palladium powder and ingots.
• North American Palladium (NYSE: PAL), Canada's largest producer of palladium operating the Lac des Iles palladium mine near Thunder Bay, Ontario.
• Stillwater Mining (NYSE: SWC), a major North American palladium miner in Montana.^[95]

Exchange-traded products

WisdomTree Physical Palladium (LSE: PHPD) is backed by allocated palladium bullion and was the world's first palladium ETF. It is listed on the London Stock Exchange as PHPD,^[96] Xetra Trading System, Euronext and Milan. ETFS Physical Palladium Shares (NYSE: PALL) is an ETF traded on the New York Stock Exchange.

Bullion coins and bars

See also: Palladium coin

A traditional way of investing in palladium is buying bullion coins and bars made of palladium. Available palladium coins include the Canadian Palladium Maple Leaf, the Chinese Panda, and the American Palladium Eagle. The liquidity of direct palladium bullion investment is poorer than that of gold and silver because there is low circulation of palladium coins.^[97]

See also

• 2000s commodities boom
• 2020s commodities boom
• Bullion
• Bullion coin
• Inflation hedge
• Pseudo palladium
• Rare materials as an investment:
  • Silver as an investment
  • Gold as an investment
  • Platinum as an investment
  • Diamonds as an investment

References

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2. Palladium(V) has been identified in complexes with organosilicon compounds containing pentacoordinate palladium; see Shimada, Shigeru; Li, Yong-Hua; Choe, Yoong-Kee; Tanaka, Masato; Bao, Ming; Uchimaru, Tadafumi (2007). "Multinuclear palladium compounds containing palladium centers ligated by five silicon atoms". Proceedings of the National Academy of Sciences. 104 (19): 7758–7763. doi:10.1073/pnas.0700450104. PMC 1876520. PMID 17470819.
3. Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
4. Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
5. Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
6. Hammond, C. R. (2004). "The Elements". Handbook of Chemistry and Physics (81st ed.). CRC press. ISBN 978-0-8493-0485-9.
7. B. Strizker, Phys. Rev. Lett., 42, 1769 (1979).
8. "Atomic Weights and Isotopic Compositions for Palladium (NIST)". Nist. 23 August 2009. Retrieved 12 November 2009.
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• Palladium at The Periodic Table of Videos (University of Nottingham)
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• Special Market Report on Palladium and Precious Metals
• "Palladium" . Encyclopædia Britannica. Vol. 20 (11th ed.). 1911. pp. 636–637.