![]() Sodium is used in a wide array of industries where it’s used to prepare sodium compounds such as common salt, baking soda, borax, sodium nitrate, etc. Also, the pure form of sodium can be obtained by electrolysis of molten sodium chloride or thermal decomposition of sodium azide. The first commercial quantities of sodium were produced by the Deville process that includes thermal reduction of sodium carbonate with carbon at 1,100 degrees Celsius. Among these mineral compounds, halite (sodium chloride salt) is the mineral from which sodium is most often obtained by mining. Hence, element 11 is often found in many mineral ores, such as soda niter, amphibole, rock salt, feldspars, zeolite, cryolite, and sodalite. As a result, it can rarely be found in nature in its pure, elemental form. Sodium is one of the most reactive elements of the periodic table. It also occurs in spring water and alkaline and salty lakes. On our planet, oceans are one of the richest sources of sodium. Before this process, the atoms of neon are formed by the carbon atoms consolidated during nuclear fusion reactions. It’s formed when atoms of neon gain a proton. Sodium has been traced in the aforementioned celestial objects in both its atomic and ionic form. The great English chemist also succeeded in obtaining scientific evidence for the sodium’s reaction with water that produced hydrogen as a result.ĭespite the lower density in comparison to the other metal elements, Sir Davy held his opinion that it should be also classified as a metal, pointing out the fact that the platinum is nearly four times as heavy as tellurium, as well as the great differences of the chemical properties among the metal elements.Ĭopious quantities of sodium can be found in the heavy stars, the Sun, as well as in the region between the stars, made up of gaseous clouds and solid particles. The electrolysis was powered by three batteries made by this Cornish inventor.ĭuring the experiment, Sir Davy observed a liquid substance at the wire electrode immersed in sodium hydroxide which turned into a solid and silvery-lustrous metal when exposed to room temperature. For this, he conducted electrolysis of caustic soda which resulted in the pure form of sodium for the first time in science. Intrigued by his discovery of the electrical nature of the chemical bonding, Sir Davy came up with the idea that he could use this electricity for isolating the chemical elements from the compounds. In 1807, the English chemist Sir Humphry Davy (1778 – 1829) became the first scientist who succeeded in preparing elemental sodium. ![]() Sodium metals float in water due to their extremely low density. ![]() This chemical reaction also produces sodium hydroxide and hydrogen gas. In contact with water, sodium creates an extremely volatile reaction that results in an explosion that releases a large amount of heat. This member of the alkali metals family of elements has an electronegativity of 0.9 according to Pauling, whereas the atomic radius according to van der Waals is 0.196 nm. Even though the density of alkali metals increases with the increase of the atomic number, sodium has a higher density in comparison to potassium. It also emits a brilliant yellow flame in the reaction with any of the major air components: nitrogen (N2), oxygen (O2), carbon dioxide (CO2), water (H2O). When exposed to air, sodium metal tarnishes and the substance loses its silvery luster. With the periodic table symbol Na, atomic number 11, atomic mass of 22.990 (23) g.mol-1, and electron configuration 3s1, sodium is soft, easily malleable, silvery-white metal with a bright luster that can be dented with any harder object. Medieval Latin: sodanum symbol from Latin natrium. Lightweight, malleable, silvery-white metal. Chemical and Physical Properties of Sodium PropertyĪ silvery-white alkali metal with a bright lusterįew uses for pure metal compounds in medicine, agriculture, photography.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |