![]() ![]() In rubidium bcc crystals, their Rb atoms interact with each other thanks to the metallic bond. This structure is characteristic for alkali metals, which are light and tend to float on water except from rubidium down (cesium and francium). Rubidium atoms are arranged in such a way as to establish a crystal with a body centered cubic structure (bcc, for its acronym in English body centered cubic). Reacts with hydrogen to form its corresponding hydride:Īnd also with halogens and sulfur explosively:Īlthough rubidium is not considered a toxic element, it is potentially dangerous and poses fire hazards when it comes in contact with water and oxygen. Although it does not react with acids and bases, it does react violently with water, generating rubidium hydroxide and hydrogen gas: Reacts with oxygen to form a mixture of peroxides (Rb 2OR 2) and superoxides (RbO 2). If heated, it also emits a violet flame (top image), which is a positive test for Rb ions +. As soon as it is exposed to the air, it begins to burn, and if it is struck, it shoots light sparks. Rubidium is one of the most reactive alkali metals, after cesium and francium. Therefore, even talc is harder than metallic rubidium. Third: 3859.4 kJ / mol (Rb 3+ gaseous) Atomic radioĠ.3. Heat of fusionĠ.82 on the Pauling scale Electronic affinity The density of rubidium is higher than that of water, so it will sink while reacting violently with it. It is usually packaged in glass ampoules, within which an inert atmosphere predominates that protects it from reacting with air. Physical and chemical properties Appearance To achieve this they tried in two ways: apply electrolysis to rubidium chloride, or heat a salt that is easier to reduce, such as its tartrate. ![]() Identifying and isolating a salt of the new element rubidium, the German chemists only needed to reduce it to its metallic state. Later, Bunsen and Kirchhoff managed to separate the Rb 2PtCl 6 from K 2PtCl 6 by fractional crystallization to finally reduce it to its chloride salt using hydrogen. That is why they baptized it with the name 'rubidus' which means 'dark red'. The emission spectrum of this new element is characterized by having two well-defined lines in the red region. However, when they studied its spectrum by burning it in the Bunsen burner, they realized that it exhibited emission lines that did not coincide with any other element at that time. They started from 150 kg of lepidolite mineral, which they treated with chloroplatinic acid, H 2PtCl 6, to precipitate potassium hexachloroplatinate, K 2PtCl 6. ![]() Their object of study was the mineral lepidolite, whose sample was collected from Saxony, Germany. To do this, they used the Bunsen burner and the spectroscope, invented two years earlier, as well as analytical precipitation techniques. Rubidium was discovered in 1861 by the German chemists Robert Bunsen and Gustav Kirchhoff, using spectroscopy. ![]() This is why rubidium is sometimes regarded as an underrated or under-studied metal. One of them is the atomic clock, solar cells and magnetometers. On the other hand, both ions give off a violet flame in the heat of the lighter.ĭue to its high cost, its applications are not based too much on the synthesis of catalysts or materials, but as a component for various devices with theoretical physical bases. Even so, rubidium supplements have been used to alleviate certain medical conditions such as depression and epilepsy. The organism "confuses" the K ions + by those of Rb + however, rubidium is not an essential element to date, as its role in metabolism is unknown. Not only in geochemical matters it forms a duo with potassium, but also in the field of biochemistry. It shows a clear tendency to associate with potassium in its minerals, being found as impurities. Rubidium is distinguished by being a more expensive metal than gold itself not so much because of its scarcity, but because of its wide mineralogical distribution in the earth's crust and the difficulties that arise when isolating it from potassium and cesium compounds. There have been experiments in which blisters burst where it is stored (bottom image) to fall and explode in bathtubs. It also reacts with it more explosively compared to lithium, sodium and potassium. It is the first of the alkali metals that, despite being not very dense, sinks in water. It is one of the most reactive metals that exist. Its name sounds similar to ruby, and it is because when it was discovered its emission spectrum showed characteristic lines of deep red color. The rubidium It is a metallic element that belongs to group 1 of the periodic table: that of the alkali metals, being represented by the chemical symbol Rb. Decay scheme of K-Ar, U-Pb and Sm-Nd, petrogenetic implications-part A Content ![]()
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