| Discovery date | 1923 |
| Discovered by | George Charles de Hevesy and Dirk Coster |
| Origin of the name | The name is derived from the Latin name for Copenhagen, 'Hafnia' |
| Allotropes | - |
Hf
Hafnium
72
178.486
| Group | 4 | Melting point | 2233°C, 4051°F, 2506 K |
| Period | 6 | Boiling point | 4600°C, 8312°F, 4873 K |
| Block | d | Density (g cm−3) | 13.3 |
| Atomic number | 72 | Relative atomic mass | 178.486 |
| State at 20°C | Solid | Key isotopes | 177Hf, 178Hf, 180Hf |
| Electron configuration | [Xe] 4f145d26s2 | CAS number | 7440-58-6 |
| ChemSpider ID | 22422 | ChemSpider is a free chemical structure database | |
Image explanation
The image is based on the civic coat of arms for the city of Copenhagen, which gives the element its name.
Appearance
A shiny, silvery metal that resists corrosion and can be drawn into wires.
Uses
Hafnium is a good absorber of neutrons and is used to make control rods, such as those found in nuclear submarines. It also has a very high melting point and because of this is used in plasma welding torches.
Hafnium has been successfully alloyed with several metals including iron, titanium and niobium.
Hafnium oxide is used as an electrical insulator in microchips, while hafnium catalysts have been used in polymerisation reactions.
Biological role
Hafnium has no known biological role, and it has low toxicity.
Natural abundance
Most zirconium ores contain around 5% hafnium. The metal can be prepared by reducing hafnium tetrachloride with sodium or magnesium.
In 1911, Georges Urbain reported the discovery of the missing element below zirconium in the periodic table, but he was wrong and the search continued. It was finally discovered by George Charles de Hevesy and Dirk Coster at the University of Copenhagen in 1923. It was found in a zirconium mineral, a Norwegian zircon, but it had proved very difficult to separate it from zirconium and this explained why hafnium remained undiscovered for so long.
Other zirconium minerals were now examined by Hevesy, and some were found to contain as much as five per cent of hafnium. (It meant the atomic weight of zirconium was wrong and hafnium-free material had to be produced in order for this to be determined.)
The first pure sample of hafnium itself was made in 1925 by decomposing hafnium tetra-iodide over a hot tungsten wire.
| Atomic radius, non-bonded (Å) | 2.23 | Covalent radius (Å) | 1.64 |
| Electron affinity (kJ mol−1) | 1.351 |
Electronegativity (Pauling scale) |
1.3 |
|
Ionisation energies (kJ mol−1) |
1st
658.519
2nd
1447
3rd
2248.1
4th
3215.86
5th
-
6th
-
7th
-
8th
-
|
||
| Common oxidation states | 4 | ||||
| Isotopes | Isotope | Atomic mass | Natural abundance (%) | Half life | Mode of decay |
| 174Hf | 173.940 | 0.16 | 2.0 x 1015 y |
|
|
| 176Hf | 175.941 | 5.26 | - | - | |
| 177Hf | 176.943 | 18.6 | - | - | |
| 178Hf | 177.944 | 27.28 | - | - | |
| 179Hf | 178.946 | 13.62 | - | - | |
| 180Hf | 179.947 | 35.08 | - | - | |
|
|
|
Specific heat capacity (J kg−1 K−1) |
144 | 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 Hafnium Podcast |
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Transcript :
Chemistry in its element: hafnium (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, super alloys, nuclear reactors and space rockets. Just some of the reasons that this week's uncommon and unknown element Hafnium is cherished by scientists worldwide. Here's Eric Scerri. Eric Scerri Today I am going to talk about an uncommon element that is also not very well known. However it has a rather interesting history and some important commercial applications including its use in the nuclear power industry and in the making of super-alloys. The element is number 72 in the periodic table, and is called hafnium. It takes its name from hafnium, the old Latin name for Copenhagen which is the city in which it was first isolated in 1922. But first let me back-track a little. In 1913, the physicist Henry Moseley, working in Manchester and later Oxford, discovered an experimental method for ordering the elements according to their atomic numbers. Prior to this work the elements in the periodic table had been ordered by using their atomic weights, which gave rise to a series with uneven gaps between each element. As a result, nobody could be sure how many elements remained to be discovered. All this changed following Moseley's discovery because atomic number increases in whole number steps as one moves through the periodic table. One of the gaps that opened up, was between element 71, lutetium, and element 73, tantalum. Moreover this particular case was complicated by the fact that it was not clear if element 72 would turn out to be a transition metal, or perhaps a rare earth element, since element 72 falls at the boundary between these two types of elements. Some chemists thought the element would be a rare earth element and carried out many fruitless searches for the element among minerals containing rare earths. But some other chemists suggested that the new element would be a transition metal. The chemical argument for this was quite simple. According to some versions of the periodic table, element 72 fell underneath titanium and zirconium in the periodic table, and both of these elements were known transition elements. Then an argument from physics was proposed by Niels Bohr, one of the founders of quantum theory. According to the electronic configuration that Bohr predicted for element 72 he also agreed that it had be a transition metal. In 1923 Coster and Hevesy a couple of young researchers in Bohr's institute decided to try to isolate the element as a test of Bohr's theory. In order to do this they followed the chemists' suggestion and decided to look among the ores of zirconium. Within just a few weeks they succeeded by examining some Norwegian zircon and by detecting the X-ray spectral line frequencies expected for this element. It was the discovery of one of the only six then remaining gaps in the periodic table. It also turned out to be the one but last discovery of any naturally occurring element, the last one being rhenium a few years later. Hafnium is not all that uncommon compared to many other exotic elements. It occurs to the extent of 5.8 ppm of the Earth's upper crust by weight. The reason why it took a long time to isolate is that its atoms have almost the identical size to those of zirconium, along with which it typically occurs in minerals. This makes it difficult to separate from zirconium. But these days a number of methods of extraction have been developed and hafnium has found many of applications because of its rather specific properties. It is a shiny, silvery metal that is corrosion resistant to a remarkable degree. More important perhaps, it has a very high ability to capture neutrons which renders it ideal for making control rods in nuclear reactors, especially those that need to operate under harsh conditions such as today's pressurized water reactors. Hafnium is also very good at forming super-alloys, which can withstand very high temperatures and has found applications in making a variety of parts for space vehicles. In terms of regular compounds rather than alloys, hafnium carbide has the highest melting point, of any compound consisting of just two elements, at just under 3,9900C. Moving up to compounds of three elements, the mixed carbide of tungsten and hafnium has the single highest melting point of any known compound at 41250C. Hafnium is not cheap given how difficult it is to extract and because of its relative scarcity. But there are some cases where one just has to pay the price! In the case of nuclear reactors for example, it costs in excess of a million dollars just for the neutron absorbing hafnium rods. On my recent trip to Copenhagen I spent a long time looking for the famous little mermaid that is symbolic of the city. When I found it I was surprised to see that it is rather insignificant but this did not seem to lessen the special attention that it held from tourists from all over the world. I think it's a little bit like the metal hafnium, first discovered in the mermaid's city of Copenhagen. It too seems somewhat insignificant at first sight and yet it holds the attention of a variety of scientists because of its rather special properties. Meera Senthilingam The ability to capture neutrons and the highest melting point of any compound, you can see why scientists consider this element as special as the little mermaid. That was Eric Scerri revealing the powers of Hafnium. Now next week, we meet the King of the elements. Brian Clegg Forget 10 Downing Street or 1600 Pennsylvania Avenue, the most prestigious address in the universe is number one in the periodic table, hydrogen. In science, simplicity and beauty are often equated - and that makes hydrogen as beautiful as they come, a single proton and a lone electron making the most compact element in existence. Meera Senthilingam And Brian Clegg will be revealing the beauty of hydrogen in next week's Chemistry in its element. Until then, thanks for listening, I'm Meera Senthilingam from the nakedscientists.com and I'll see you next week. (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.
