| Discovery date | 1913 |
| Discovered by | Kasimir Fajans and Otto Göhring |
| Origin of the name | The name is derived from the Greek 'protos', meaning first, as a prefix to the element actinium, which is produced through the radioactive decay of proactinium. |
| Allotropes |
|
Pa
Protactinium
91
231.036
| Group | Actinides | Melting point | 1572°C, 2862°F, 1845 K |
| Period | 7 | Boiling point | 4000°C, 7232°F, 4273 K |
| Block | f | Density (g cm−3) | 15.4 |
| Atomic number | 91 | Relative atomic mass | 231.036 |
| State at 20°C | Solid | Key isotopes | 231Pa |
| Electron configuration | [Rn] 5f26d17s2 | CAS number | 7440-13-3 |
| ChemSpider ID | 22387 | ChemSpider is a free chemical structure database | |
Image explanation
The icon is based on the Japanese monogram for ‘ichi’ – number one. This reflects the origin of the element’s name from the Greek ‘protos’, meaning first.
Appearance
A silvery, radioactive metal.
Uses
Protactinium is little used outside of research.
Biological role
Protactinium has no known biological role. It is toxic due to its radioactivity.
Natural abundance
Small amounts of protactinium are found naturally in uranium ores. It is also found in spent fuel rods from nuclear reactors, from which it is extracted.
Mendeleev said there should be an element between thorium and uranium, but it evaded detection. Then, in 1900, William Crookes separated an intensely radioactive material from uranium, but did not identify it. In 1913, Kasimir Fajans and Otto Göhring showed that this new element decayed by beta-emission and it existed only fleetingly. We now know it is a member of the sequence of elements through which uranium decays. It was the isotope protactinium-234, which has a half-life of 6 hours 42 minutes.
A longer-lived isotope was separated from the uranium ore pitchblende (uranium oxide, U3O8) in 1918 by Lise Meitner at the Kaiser-Wilhelm Institute in Berlin. This was the longer-lived isotope protactinium-231, also coming from uranium, and its half-life is 32,500 years.
In 1934, Aristid von Grosse reduced protactinium oxide to protactinium metal by decomposing its iodide (PaF5) on a heated filament.
| Atomic radius, non-bonded (Å) | 2.43 | Covalent radius (Å) | 1.84 |
| Electron affinity (kJ mol−1) | Unknown |
Electronegativity (Pauling scale) |
1.5 |
|
Ionisation energies (kJ mol−1) |
1st
568.3
2nd
-
3rd
-
4th
-
5th
-
6th
-
7th
-
8th
-
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| Common oxidation states | 5, 4 | ||||
| Isotopes | Isotope | Atomic mass | Natural abundance (%) | Half life | Mode of decay |
| 231Pa | 231.036 | 100 | 3.25 x 104 y | α | |
| > 2 x 1017 y | sf | ||||
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Specific heat capacity (J kg−1 K−1) |
Unknown | Young's modulus (GPa) | Unknown | |||||||||||
| Shear modulus (GPa) | Unknown | Bulk modulus (GPa) | Unknown | |||||||||||
| Vapour pressure | ||||||||||||||
| Temperature (K) |
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| Pressure (Pa) |
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| Listen to Protactinium Podcast |
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Transcript :
Chemistry in its element: protactinium (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 we've got an element whose origin and location in the periodic table seems to be causing some complications. To tell us more about the mysteries of protactinium here's Eric Scerri: Eric Scerri In 1871 the discoverer of the periodic table, Dimitri Mendeleev, made the following prediction among several others. I quote: "Between thorium and uranium we can further expect an element with an atomic weight of about 235. This element should form a highest oxide X2O5, like niobium and tantalum to which it should be analogous." The modern atomic weight for the predicted element, or protactinium as it is now known, is close to 231. Even though this seems reasonably accurate, Mendeleev was somewhat unlucky regarding this atomic weight since he was not to know that protactinium is a member of only four 'pair reversals' in the entire periodic table. This situation occurs when two elements need to be reversed contrary to their atomic weights in order to order them correctly. When atomic number was discovered it turned out to be a better ordering principle than atomic weight for the elements in the periodic table. All four known pair reversals, including the one concerning protactinium and thorium were suddenly resolved. Even though protactinium has a lower atomic weight than thorium it should be placed after thorium because of its greater atomic number. But it appears that Mendeleev's brief predictions were broadly fulfilled since the element does indeed show an analogy with tantalum in forming Pa2O5 as its highest and most stable oxide. Nevertheless protactinium also shows a strong horizontal analogy with thorium and uranium in also displaying the +4 oxidation state, something that Mendeleev does not seem to have anticipated. Finally, as Mendeleev also correctly predicted protactinium occurs with uranium, and more specifically in the ore called pitchblende. But whereas uranium and thorium were isolated in 1789 and 1828 respectively, it was not until the twentieth century before protactinium, was first discovered. Of course it depends on what one really means by the discovery of an element. Does it mean somebody realizing that a mineral contains a new element, or does it mean the first time an element is actually isolated? Depending on what choice is made the discovery of protactinium can be assigned to different scientists. And in the case of protactinium there is an even further complication. In the year 1900 the English scientist and inventor Sir William Crookes pointed out that a new radioactive substance was present in some ores of uranium and he called this substance uranium-X. Uranium-X turned out to be two different substances later called UX-1 and UX-2 of which the second, UX-2 was first isolated by the Polish chemist Kasimir Fajans in 1913. This was a very short-lived isotope of 234Pa with a half-life of just over one minute. Fajans called the new element brevium after its short half-life. In 1917 the German physicist Lise Meitner isolated a more stable isotope of the element, 231Pa with a vastly longer half-life of about 33,000 years. At this point Fajans withdrew the name brevium since the custom was to name an element according to longest-lived isotope. Meitner than chose the somewhat awkward sounding name of protoactinium which was eventually abbreviated to protactinium. The name she chose refers to the fact that this element is the progenitor of element 89 or actinium, which is formed when protactinium decays via the loss of an alpha particle. In the very same year, the same isotope, 231Pa, was independently isolated by Frederick Soddy, who had first coined the term isotope, and his colleague John Cranston when they were working together in Glasgow. Protactinium is a highly radioactive and highly toxic element with yet no commercial applications but nevertheless of some scientific interest. For example, a measurement of the ratio of 231Pa and 230Th in ocean sediments allows scientists to reconstruct the movements of bodies of North Atlantic water that took place during the melting of the last ice-age. In 1961 the Atomic Energy Authority in Britain produced a concentrated mass of 125 grams of protactinium after processing 60 tons of radioactive waste. For many years this has remained as the only significant supply of protactinium which has provided samples of the element to labs around the world. Meera Senthilingam So a highly radio active and toxic element whose origin and isolation had scientists mystified. That was Eric Scerri from the University of California, Los Angeles, with the perplexing tale of protactinium. Now next week an element that's definitely got one up on the rest when it comes to history. Brian Clegg Perhaps iridium's best-known claim to fame is as a clue in a piece of a 65 million-year-old Crime Scene Investigation. The concentration of iridium in meteorites is considerably higher than in rocks on the Earth. One class of meteorite, called chondritic (meaning they have a granular structure) still has the original levels of iridium that were present when the solar system was formed. Meera Senthilingam And join Brian Clegg to find out how Iridium can inform us about life on earth in next week's Chemistry in its element. Until then I'm Meera Senthilingam 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.
