![]() Key properties for the Group 1 elements for ICP-MS analysis Table 1 shows some key properties of these elements with regard to their analysis by ICP-MS. These elements are all easily ionized in an argon ICP and generate large populations of singly charged ions. It decays into radium-223 through beta decay or into astatine-219 through alpha decay. Francium’s most stable isotope, 223Fr, has a half-life of around 22 minutes. This element takes its name from the country where it was discovered, France. The last member of Group 1 is the unstable element francium (Fr), discovered by Marguerite Perey at the Curie Institute in Paris in 1939 when she was researching the radioactive decay of actinium-227. The bright redlines in its emission spectrum led them to choose a name derived from the Latin word “rubidus,” meaning “deep red.” It was also Bunsen and Kirchhoff who discovered rubidiumin 1861during their analysis of the mineral lepidolite using flame spectroscopy. Their identification was based upon two distinctive bright blue lines in the spectrum of Cs, leading them to coin the name “caesium,” from the Latin “caesius,” meaning “heavenly blue.” The element derives its name from the Greek word “lithos,” meaning “stone,” because it was found in the mineral petalite (LiAlSi 4O 10).Ĭaesium (US, cesium) was discovered by Robert Bunsen and Gustav Kirchhoff, in Heidelberg, Germany, in 1860 during their analysis of mineral water samples from Durkheim using flame spectroscopy. Lithium was detected by the Swedish chemist Johan August Arfvedson in 1817, but actually first isolated by William Thomas Brande and Sir Humphrey Davy through the electrolysis of lithium oxide (Li 2O) in 1821. The origin of the name comes from the Latin word for sodium carbonate, ‘natrium.’ It was also Davy who discovered sodium later in 1807, again using electrolysis, but this time of molten sodium hydroxide. This element derives its name from the Arabic word “al-qali,” meaning alkali, with the symbol K coming from the Latin word “kalium.” Davy extracted the element from caustic potash (potassium hydroxide) using electrolysis – potassium was actually the first metal to be isolated using this technique. The first member of the group to be identified was potassium, discovered by the English chemist, Sir Humphrey Davy, in 1807. The stable alkali metals (Group 1 of the Periodic Table) consist of lithium (Li), sodium (Na), potassium (K), rubidium (Rb) and caesium (Cs), with the unstable francium (Fr) completing the group. Our expedition starts with the elements of Group 1 – the alkali metals. I’ll discuss how this technique can be applied to the members of the various Periodic Table groups in terms of what parameters work best for them, what pitfalls you need to watch out for and how you can avoid these problems and successfully achieve good quality elemental analysis in your laboratory. I have previously discussed these issues in detail in my blog post series “How to Improve Your ICP-MS Analysis” parts 1, 2 and 3.īuilding on these earlier articles, in this blog post series, I will take you on a journey of exploration through the Periodic Table, from the perspective of ICP-MS. ![]() Leading the charge to meet these requirements has been ICP-MS, but the pursuit of these goals has uncovered a number of challenges for this technique, including interference, contamination, and sample-to-sample washout issues. With this increase in the utilization of elemental analysis, instrumentation has come a demand for ever-higher sensitivity and ever-lower detection limits. From the early days of atomic absorption spectrometry (AAS) in the 1950s to the present generation of sensitive and fast inductively coupled plasma optical emission and mass spectrometers (ICP-OES and ICP-MS), detection and quantification of metals and semi-metals has expanded to encompass every area of analytical science, from geology and environmental analysis to clinical and life science research. Since Dmitry Mendeleev first proposed that different elements could be related together in rows and columns according to similarities in their properties in 1869, the Periodic Table has grown to include various stable elements that were unknown in Mendeleev’s time, as well as a kaleidoscope of exotic short-lived nuclides produced in particle accelerator experiments.Īs the Periodic Table has evolved, so have techniques for measuring the elements within it. The Periodic Table is one of the most familiar creations in the world of chemistry.
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