However, as it melts the density decreases to 2.375 g/cm3. Principally, the element assumes a solid-state and has a density of 2.64 g/cm2 at room temperature.
As such, the metal assumes a pale-yellow appearance. Strontium is a silvery-white, soft element that rapidly reacts in the air (oxygen) to form a thin film of yellow precipitate (SEO). Also, it is fundamental in “the manufacture of ceramics and specialty glass” (CHEMICAL, PHYSICAL and RADIOLOGICAL INFORMATION”). Moreover, one major application of strontium is in the production of cathode-ray tubes meant for color television. The table below shows a summary of the radiological properties of strontium isotopes.ĭespite its carcinogenicity, one of the strontium radioactive isotopes is vital in medical studies. Fundamentally, unlike other radioactive isotopes, strontium decays by emitting a beta together with the creation of a progeny product- virtually a beta emitter. 90Sr’s half-life dwarfs 89Sr (51 days) by more than 200 folds.
Nevertheless, between the two isotopes, 90Sr is the more potent one thanks to its relatively long half-life (twenty-nine years). These two radioactive isotopes are synonymous with the human health fraternity owing to their carcinogenicity. This process is depicted by the below nuclear equation:Ģ35U + 1n 89Sr + 90Sr + other fission by-products (CHEMICAL, PHYSICAL and RADIOLOGICAL INFORMATION”) These emanate from a nuclear fission process of radioactive isotopes (239Pu, 235U or, 238U) after bombardment with a high-energy neutron. Of great importance in radiology are isotopes 89Sr and 90Sr. The rest are artificial isotopes and, are a consequence of radioactivity. The naturally occurring isotopes include “84Sr (0.56%), 86Sr (9.86%), 87Sr (7.0%) and 88Sr (82.58%)” (CHEMICAL, PHYSICAL and RADIOLOGICAL INFORMATION”) are the only stable isotopes. Strontium boasts a total of 26 isotopes of which 4 happen naturally. Under ideal environmental conditions, the later oxidation state is steady enough vital for practical use since its reaction with both water and oxygen is feasible. Principally, elemental strontium can exist either as 0 or +2 oxidation states. To be specific, the duo processes achieve 97 and 98% SrCo3 respectively. With regards to commercial production contemporary processes including soda and black ash, methods are known to achieve near-perfect production of strontium compounds from a mineral. Naturally, strontium exists as a mineral compound and the chief sources of commercial interest include strontianite (SrCo3) and celestite (SrSo4). It has a high affinity for oxygen thus it exists as a compound of strontium oxide (SEO). However, because of its reactivity in the air, the element rarely exists as a pure element. To this end, using electrolysis of a molten compound (strontium chloride), Davy was able to isolate pure metal of strontium from the compound. However, it was until two decades later that a pure element of strontium was prepared by one Humphrey Davy, an English chemist. Its existence was unearthed in the year 1790 by one Adair Crawford, an Irish physician. The name strontium is owed to a Scotland village, Strontia, where the element was discovered. The elemental strontium is chemically denoted as Sr, has an atomic number of 38 and an atomic mass of 87.62 AMU. beryllium, magnesium, and calcium), and less reactive than all the members that come below it in the group e.g. Precisely, strontium is more reactive than all the members above it in the group (e.g. Principally, on the periodic table strontium occupies a central position in the group thus it’s either more or less reactive than members of its group. These members have two electrons on their outer energy level hence the name Group II. Strontium is a vital chemical element found in Group II (II A) of the periodic table.įundamentally, together with strontium, the entire members of this group including radium, barium, calcium, magnesium, and beryllium among others have a common atomic structure that makes them members of this group (alkaline earth metals).
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