| Discovery date | 1803 |
| Discovered by | William Hyde Wollaston |
| Origin of the name | Palladium is named after the asteroid Pallas, in turn named after the Greek goddess of wisdom, Pallas. |
| Allotropes |
|
Pd
Palladium
46
106.42
| Group | 10 | Melting point | 1554.8°C, 2830.6°F, 1828 K |
| Period | 5 | Boiling point | 2963°C, 5365°F, 3236 K |
| Block | d | Density (g cm−3) | 12.0 |
| Atomic number | 46 | Relative atomic mass | 106.42 |
| State at 20°C | Solid | Key isotopes | 106Pd |
| Electron configuration | [Kr] 4d10 | CAS number | 7440-05-3 |
| ChemSpider ID | 22380 | ChemSpider is a free chemical structure database | |
Image explanation
The image represents the asteroid Pallas, after which the element is named. In the background are 20th-century star charts.
Appearance
A shiny, silvery-white metal that resists corrosion.
Uses
Most palladium is used in catalytic converters for cars. It is also used in jewellery and some dental fillings and crowns. White gold is an alloy of gold that has been decolourised by alloying with another metal, sometimes palladium.
It is used in the electronics industry in ceramic capacitors, found in laptop computers and mobile phones. These consist of layers of palladium sandwiched between layers of ceramic.
Finely divided palladium is a good catalyst and is used for hydrogenation and dehydrogenation reactions. Hydrogen easily diffuses through heated palladium and this provides a way of separating and purifying the gas.
Biological role
Palladium has no known biological role. It is non-toxic.
Natural abundance
Palladium has been found uncombined in nature, in Brazil, but most is found in sulfide minerals such as braggite. It is extracted commercially as a by-product of nickel refining. It is also extracted as a by-product of copper and zinc refining.
As early as 1700, miners in Brazil were aware of a metal they called ouro podre, ‘worthless gold,’ which is a native alloy of palladium and gold. However, it was not from this that palladium was first extracted, but from platinum, and this was achieved in 1803 by William Wollaston. He noted that when he dissolved ordinary platinum in aqua regia (nitric acid + hydrochloric acid) not all of it went into solution.
It left a residue from which he eventually extracted palladium. He did not announce his discovery but put the new metal on sale as a ‘new silver’. Richard Chenevix purchased some, investigated it, and declared it to be an alloy of mercury and platinum. In February 1805 Wollaston revealed himself as its discoverer and gave a full and convincing account of the metal and its properties.
| Atomic radius, non-bonded (Å) | 2.10 | Covalent radius (Å) | 1.30 |
| Electron affinity (kJ mol−1) | 54.225 |
Electronegativity (Pauling scale) |
2.20 |
|
Ionisation energies (kJ mol−1) |
1st
804.389
2nd
1874.71
3rd
3177.26
4th
-
5th
-
6th
-
7th
-
8th
-
|
||
| Common oxidation states | 4, 2, 0 | ||||
| Isotopes | Isotope | Atomic mass | Natural abundance (%) | Half life | Mode of decay |
| 102Pd | 101.906 | 1.02 | - | - | |
| 104Pd | 103.904 | 11.14 | - | - | |
| 105Pd | 104.905 | 22.33 | - | - | |
| 106Pd | 105.903 | 27.33 | - | - | |
| 108Pd | 107.904 | 26.46 | - | - | |
| 110Pd | 109.905 | 11.72 | - | - | |
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Specific heat capacity (J kg−1 K−1) |
244 | Young's modulus (GPa) | 46 | |||||||||||
| Shear modulus (GPa) | 18 | Bulk modulus (GPa) | 33 | |||||||||||
| Vapour pressure | ||||||||||||||
| Temperature (K) |
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| Pressure (Pa) |
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| Listen to Palladium Podcast |
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Transcript :
Chemistry in its element: palladium (Promo) You're listening to Chemistry in its element brought to you by Chemistry World, the magazine of the Royal Society of Chemistry. (End promo) Meera Senthilingam This week, an element whose discovery was announced in a very unique way. So to explain more above the discovery and chemistry of palladium, here's Simon Cotton. Simon Cotton For the first 5 years of my life, I lived in the Norfolk market town that was the birthplace of the discoverer of palladium, William Hyde Wollaston. When he isolated this metal in 1802, he did something quite unique. Instead of announcing it in a reputable scientific journal, he described its properties in an anonymous leaflet, displayed in the window of a shop in Gerrard Street, Soho, in April 1803. Entitled 'PALLADIUM; OR, NEW SILVER', this handbill described properties of the new element, giving its density and several of its chemical properties, concluding with the announcement that it was sold only at that shop 'In Samples of Five Shillings, Half a Guinea & One Guinea each.' No one was able to refute Wollaston's claim for a new element, but it was not until 1805 that he published his discovery in a scientific journal. Palladium is a remarkable metal, not least because it will absorb over 900 times its volume of hydrogen gas. The hydrogen is released again when the metal is heated, so this can be a rather cunning way of weighing hydrogen. And because palladium won't absorb any other gas, you can use this property to purify hydrogen. At the bottom of our hearts, we know that the age of cheap energy is over. Quite apart from worries about the greenhouse effect and global warming, oil is running out, and the search is on for green alternatives, and palladium is concerned in the most controversial claim that has been made in this area. Life on Earth relies on the sun. The sun produces energy by fusing hydrogen atoms together to produce helium, a process that requires extremely high temperatures. On March 23 1989, two scientists working in the USA, Martin Fleischmann and Stanley Pons, reported results of room-temperature electrolysis of heavy water using a platinum anode and a palladium cathode. They claimed to have produced excess energy, and suggested that it arose from nuclear fusion reactions. This was seen as a source of cheap energy, possibly solving the world's energy problems. When hydrogen molecules first come into contact with palladium, they are adsorbed on the surface, but then they diffuse throughout the metal. In palladium saturated with hydrogen, the molecules are extremely close together. Fleischmann and Pons believed that this closeness had led to the energy-producing nuclear fusion reactions happening. Over the last twenty years, no one has been able to reproduce this, and the reaction has passed into the realms of Voodoo Science. Palladium does however have a genuine use in 'green' energy, as a catalyst in hydrogen fuel cells. Palladium is one of a number of metals starting to be used in the fuel cells to power a host of things including cars and buses. Palladium is also widely used in catalytic reactions in industry, such as in hydrogenation of unsaturated hydrocarbons, as well as in jewellery and in dental fillings and crowns. But the main use of palladium, along with rhodium and platinum, is in the three-way catalytic converters in car exhaust systems. Untreated, car exhaust fumes contain several undesirable gases, and the purpose of the catalytic converters is to eliminate them. They are called three-way converters as they reduce three types of harmful emissions. Converting toxic carbon monoxide into carbon dioxide; the hydrocarbons in unburned fuel into carbon dioxide and water; and toxic oxides of nitrogen (which can contribute to smog and acid rain) into harmless nitrogen gas. So, that's palladium - a metal with humble beginnings that now plays a major role in industrial catalysis, powering and cleaning up after our vehicles and even makes the occasional appearance in our jewellery boxes, and even in our mouths. Meera Senthilingam Quite the catalyst that palladium! Providing energy in fuel cells, protecting our environment through catalytic converters, and providing aesthetic pleasure in jewellery and even dentistry. That was Simon Cotton, from Uppingham School in the UK, with the chemistry of palladium. Next week, an element that certainly doesn't deserve to be called boring. Louise Natrajan There is a famous quote about the lanthanides by Pimentel and Sprately from their book, Understanding Chemistry published in 1971: If you've listened to any other of the podcasts in the lanthanide series, I hope you'll agree that this is far from true. While, the most common oxidation state of the lanthanides is indeed the +3 valence state, ytterbium, the last and smallest of the lanthanides or rare earths in the series is one of the exceptions Pimentel and Sprately were talking about. Meera Senthilingam And Louise Natrajan will be revealing the true - exciting - nature of ytterbium that makes it one of the exceptions, in next week's Chemistry in its element. Until then, I'm Meera Senthilingham, and thank you for listening. (Promo) Chemistry in its element is brought to you by the Royal Society of Chemistry and produced by thenakedscientists.com. There's more information and other episodes of Chemistry in its element on our website at chemistryworld.org/elements. (End promo)
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Visual Elements images and videos
© Murray Robertson 1998-2017.
W. M. Haynes, ed., CRC Handbook of Chemistry and Physics, CRC Press/Taylor and Francis, Boca Raton, FL, 95th Edition, Internet Version 2015, accessed December 2014.
Tables of Physical & Chemical Constants, Kaye & Laby Online, 16th edition, 1995. Version 1.0 (2005), accessed December 2014.
J. S. Coursey, D. J. Schwab, J. J. Tsai, and R. A. Dragoset, Atomic Weights and Isotopic Compositions (version 4.1), 2015, National Institute of Standards and Technology, Gaithersburg, MD, accessed November 2016.
T. L. Cottrell, The Strengths of Chemical Bonds, Butterworth, London, 1954.
John Emsley, Nature’s Building Blocks: An A-Z Guide to the Elements, Oxford University Press, New York, 2nd Edition, 2011.
Thomas Jefferson National Accelerator Facility - Office of Science Education, It’s Elemental - The Periodic Table of Elements, accessed December 2014.
Periodic Table of Videos, accessed December 2014.
Derived in part from material provided by the British Geological Survey © NERC.
Elements 1-112, 114, 116 and 117 © John Emsley 2012. Elements 113, 115, 117 and 118 © Royal Society of Chemistry 2017.
Produced by The Naked Scientists.
Created by video journalist Brady Haran working with chemists at The University of Nottingham.
© Murray Robertson 1998-2017.
Data
W. M. Haynes, ed., CRC Handbook of Chemistry and Physics, CRC Press/Taylor and Francis, Boca Raton, FL, 95th Edition, Internet Version 2015, accessed December 2014.
Tables of Physical & Chemical Constants, Kaye & Laby Online, 16th edition, 1995. Version 1.0 (2005), accessed December 2014.
J. S. Coursey, D. J. Schwab, J. J. Tsai, and R. A. Dragoset, Atomic Weights and Isotopic Compositions (version 4.1), 2015, National Institute of Standards and Technology, Gaithersburg, MD, accessed November 2016.
T. L. Cottrell, The Strengths of Chemical Bonds, Butterworth, London, 1954.
Uses and properties
John Emsley, Nature’s Building Blocks: An A-Z Guide to the Elements, Oxford University Press, New York, 2nd Edition, 2011.
Thomas Jefferson National Accelerator Facility - Office of Science Education, It’s Elemental - The Periodic Table of Elements, accessed December 2014.
Periodic Table of Videos, accessed December 2014.
Supply risk data
Derived in part from material provided by the British Geological Survey © NERC.
History text
Elements 1-112, 114, 116 and 117 © John Emsley 2012. Elements 113, 115, 117 and 118 © Royal Society of Chemistry 2017.
Podcasts
Produced by The Naked Scientists.
Periodic Table of Videos
Created by video journalist Brady Haran working with chemists at The University of Nottingham.
