[4]
The discovery of gallium by the French scientist, Paul. E. L. de Boisbaudran supported Mendeleev’s ideas about the periodic table because gallium fitted into one of the gaps he had left for undiscovered elements. Mendeleev called gallium eka-aluminium (see table on next page) before it was discovered, as it was one element below aluminium in his periodic table. He even predicted its chemical and physical properties. This then gave a big boost to Mendeleev's idea of the periodic table.
Table showing Mendeleev’s predictions with properties of element 31, gallium [2]
The physical properties of gallium are considered to be unusual due to three physical properties. These three properties suggest that gallium is a non-metal.
The first is the melting point of gallium which is 29.78ºC, that’s only slightly above UK room temperature therefore gallium would become a liquid metal in hot countries like mercury. There is no known explanation about the low melting point of* gallium. But it has been suggested that it could be related to there being Ga2 molecules in the liquid.
Second, the element has a high boiling point which is 2403ºC. Gallium has the longest liquid range of any element. This is the reason why gallium is used in high temperature glass thermometers.
Third, it is denser as a liquid rather than a solid at its freezing point. This resembles a similarity between water and gallium. The explanation is also similar which is both elements have a more open structure as a liquid rather than as a liquid.
Gallium is also a semiconductor and forms covalent bonds between non-metals which also suggest that gallium is a non-metal. One of the physical properties show that gallium may be a metal, which is gallium being shinny.
‘The chemical properties of gallium are less odd than the physical ones [1]’. Gallium intimately resembles the elements above it such as aluminium. ‘Like aluminium, it dissolves in both acids and alkalis, evolving hydrogen [2]’. This gives a suggestion that gallium is a metal.
Atomic spectroscopy and UNILAC accelerator have increased our knowledge about chemical elements as these techniques have been used to find new elements which* are so rare they have never existed in nature. These two techniques have increased the chance of finding new elements and filling in the periodic table. The new elements will help scientists to understand the properties of elements.
Atomic spectroscopy involves turning the sample into an electrode for an electric arc. This would then emit a characteristic line of each element present. ‘The intensities of the lines are proportional to the concentration of atoms of each element [3]’. The technique can be used to monitor up to 20 elements.
When using the technique the user has to monitor the concentration of atoms in the element to detect if there are any change therefore relies on understanding the structure of atoms.
UNILAC accelerator involves firing a beam of relatively heavy ions from an accelerator towards a target of a heavy, stable element. ‘If the process is carried out sufficiently then the ions overcome the natural repulsion of nuclei and fuse together, creating a new element [1]’.
This technique involves nuclei’s of two different atoms fusing together to form a new element (see the diagram on the next page).
The works of chemists have changed over the last two hundred years from discovering and synthesising elements. ‘Chemists used to* believe that atoms were the smallest building blocks of matter- they could not be split into smaller particles [1]’. By early twentieth century, chemists knew that atoms consist of smaller particles.
The use of atomic spectroscopy and UNILAC accelerating has increased the chance of finding new elements. They are now able to create atoms so rare that they have never existed in nature. Although these atoms only last for a fraction of a second before disintegrating, they give scientists new insights into the very heart of matter. The discovery of elements have helped chemist understand the pattern of behaviour and properties of elements. Over the last half century, synthesising elements has become deliberate. Scientists have found elements beyond uranium and haven’t given up trying to add more elements to the periodic table.
Reference:
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Article Title: Gallium: a landmark in the history of chemistry
Publisher: Chemistry review
Edition: Volume 11, Number 2, 2001
Year Published: 2001
Author: Gordon Woods
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Article Title: Gallium
Publisher: Chemistry Review
Edition: November 2001
Author: Chris Ennis
Pages: 10-13
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Book Title: Salters advanced chemistry: Chemical Storylines, Chemical Ideas
Publisher: Heinemann
Edition: Second edition, 2000
Author: George Burton, John Holman, John Lazonby, Gwen Pilling, David Waddington
Pages: CS – 168, CI – 125
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Website address:
Webpage title: Gallium
Author: Mark Winter [The University of Sheffield and Web Elements Ltd, UK].
Summary
Mendeleev’s periodic table was arranged by increasing relative atomic mass rather than atomic number. Discovery of gallium supported Mendeleev’s theory to leave gaps for undiscovered elements. Gallium was discovered by using atomic spectroscopy. Synthesising elements involves creating an artificial element using either atomic spectroscopy or UNILAC accelerator.
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