palladium
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What is palladium?
Palladium (Pd) is a precious, gray-white metal that is the least dense and has the lowest melting point of the platinum metals. It's known for its extreme ductility and workability and doesn't tarnish at normal temperatures.
Because of its properties, palladium is used in jewelry, electrical contacts, and dental alloys. Its primary use is in automobile catalytic converters, where it helps convert pollutants like hydrocarbons, carbon monoxide, and nitrogen oxide into less harmful substances. Palladium is also used in printed-circuit components and multilayer ceramic capacitors.
Palladium is more reactive than other platinum metals, readily dissolving in nitric acid. It also has a unique ability to absorb hydrogen, holding over 900 times its volume under specific conditions, making it useful in hydrogen purification.
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What does palladium look like?
Palladium (Pd) is a precious gray-white metal that stands out as the least dense and lowest-melting among the platinum metals. It's incredibly pliable and easy to shape, and it doesn't tarnish when exposed to air at normal temperatures.
Because of its desirable properties, palladium and its alloys can replace platinum in jewelry and electrical contacts. When combined with gold in relatively small amounts, palladium yields the best white gold. It is also used in dental alloys. In addition, palladium coatings can be applied through electroplating or chemical plating in printed-circuit components and multilayer ceramic capacitors.
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Where is palladium found in nature?
Palladium, a precious gray-white metal, is found in nature alloyed with platinum and iridium in areas such as Colombia, Brazil, the Ural Mountains, and South Africa. It is one of the more abundant platinum metals, with a crustal abundance of about 0.015 part per million.
Palladium is also associated with gold, silver, copper, and nickel ores and is commercially produced as a byproduct of refining these metals. Major palladium producers include Russia, South Africa, Canada, and the United States.
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What are some common uses of palladium?
Palladium, a precious, silver-white metal, has several common uses, especially as a catalyst and in alloys. It is extremely ductile and easily worked.
Uses of palladium:
- Catalytic converters Palladium is a catalyst that converts polluting hydrocarbons, carbon monoxide, and nitrogen oxide in exhaust to water, carbon dioxide, and nitrogen.
- Jewelry Palladium and its alloys serve as substitutes for platinum in jewelry. An alloy of gold with small amounts of palladium makes the best white gold.
- Electrical contacts Palladium is used in electrical contacts.
- Dental alloys Palladium is used in dental alloys.
- Hydrogen purification Heated palladium tubes, which are impervious to other gases, are used to pass hydrogen in and out of closed gas systems or for hydrogen purification.
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Why is palladium important in making catalytic converters?
Palladium is a crucial component in catalytic converters because it acts as a catalyst that speeds up chemical reactions, helping to convert polluting hydrocarbons, carbon monoxide, and nitrogen oxide in automobile exhaust into less harmful substances like water, carbon dioxide, and nitrogen.
Often used in combination with rhodium, palladium's surfaces facilitate reactions involving hydrogen and oxygen. The ceramic catalyst supports, like pellets and honeycomb monoliths, maximize surface area for efficient conversion of the pollutants.
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How is palladium extracted and separated from other metals?
Palladium extraction and separation from other metals involves a complex chemical process. Initially, a mineral concentrate is leached with aqua regia, dissolving palladium and platinum while leaving other metals as solids. Platinum is precipitated using ammonium chloride, and palladium is then precipitated from the remaining solution by adding ammonia.
The residue is treated with molten sodium bisulfate to convert rhodium to rhodium sulfate. The rhodium is solubilized by water leaching, separated from the insolubles, and precipitated from solution by reduction with zinc powder. The residue from rhodium sulfate leaching is fused with alkali nitrate salts to convert ruthenium to soluble sodium ruthenate.
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palladium (Pd), chemical element, the least dense and lowest-melting of the platinum metals of Groups 8–10 (VIIIb), Periods 5 and 6, of the periodic table, used especially as a catalyst (a substance that speeds up chemical reactions without changing their products) and in alloys.
A precious gray-white metal, palladium is extremely ductile and easily worked. Palladium is not tarnished by the atmosphere at ordinary temperatures. Thus, the metal and its alloys serve as substitutes for platinum in jewelry and in electrical contacts; the beaten leaf is used for decorative purposes. Relatively small amounts of palladium alloyed with gold yield the best white gold. Palladium is used also in dental alloys. The chief use of palladium, however, is in automobile catalytic converters (often in combination with rhodium); the palladium serves as a catalyst to convert polluting hydrocarbons, carbon monoxide, and nitrogen oxide in the exhaust to water, carbon dioxide, and nitrogen. Palladium coatings, electrodeposited or chemically plated, have been used in printed-circuit components, and palladium is also used in multilayer ceramic capacitors.
Native palladium, though rare, occurs alloyed with a little platinum and iridium in Colombia (department of Chocó), in Brazil (Itabira, Minas Gerais), in the Ural Mountains, and in South Africa (the Transvaal). Palladium is one of the most abundant platinum metals and occurs in Earth’s crust at an abundance of 0.015 part per million. For the mineralogical properties of palladium, see native element (table). Palladium also occurs alloyed with native platinum. It was first isolated (1803) from crude platinum by the English chemist and physicist William Hyde Wollaston. He named the element in honor of the newly discovered asteroid Pallas. Palladium is also associated with a number of gold, silver, copper and nickel ores. It is generally produced commercially as a by-product in the refining of copper and nickel ores. Russia, South Africa, Canada, and the United States were the world’s leading producers of palladium in the early 21st century.
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Surfaces of palladium are excellent catalysts for chemical reactions involving hydrogen and oxygen, such as the hydrogenation of unsaturated organic compounds. Under suitable conditions (80 °C [176 °F] and 1 atmosphere), palladium absorbs more than 900 times its own volume of hydrogen. It expands and becomes harder, stronger, and less ductile in the process. The absorption also causes both the electrical conductivity and magnetic susceptibility to decrease. A metallic or alloylike hydride is formed from which the hydrogen can be removed by increased temperature and reduced pressure. Because hydrogen passes rapidly through the metal at high temperatures, heated palladium tubes impervious to other gases function as semipermeable membranes and are used to pass hydrogen in and out of closed gas systems or for hydrogen purification.
Palladium is more reactive than the other platinum metals. For example, it is attacked more readily by acids than any of the other platinum metals. It dissolves slowly in nitric acid to give palladium(II) nitrate, Pd(NO3)2, and with concentrated sulfuric acid it yields palladium(II) sulfate, PdSO4∙2H2O. In its sponge form it will dissolve even in hydrochloric acid in the presence of chlorine or oxygen. It is rapidly attacked by fused alkali oxides and peroxides and also by fluorine and chlorine at about 500 °C (932 °F). Palladium also combines with a number of nonmetallic elements on heating, such as phosphorus, arsenic, antimony, silicon, sulfur, and selenium.
A series of palladium compounds can be prepared with the +2 oxidation state; numerous compounds in the +4 state and a few in the 0 state are also known. Among the transition metals palladium has one of the strongest tendencies to form bonds with carbon. All palladium compounds are easily decomposed or reduced to the free metal. An aqueous solution of potassium tetrachloropalladate(II), K2PdCl4, serves as a sensitive detector for carbon monoxide or olefin gases because a black precipitate of the metal appears in the presence of exceedingly small amounts of those gases. Natural palladium consists of a mixture of six stable isotopes: palladium-102 (1.02 percent), palladium-104 (11.14 percent), palladium-105 (22.33 percent), palladium-106 (27.33 percent), palladium-108 (26.46 percent), and palladium-110 (11.72 percent).
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| atomic number | 46 |
|---|---|
| atomic weight | 106.40 |
| melting point | 1,554.9 °C (2,830.8 °F) |
| boiling point | 2,963 °C (5,365 °F) |
| specific gravity | 12.02 (0 °C [32 °F]) |
| oxidation states | +2, +4 |
| electron configuration | [Kr]4d10 |