Chlorine

1858 WordsAug 6, 20108 Pages
Chlorine Zachary Grindle Chemistry 1301 Professor Bott June 24, 2010 Chlorine has an atomic mass of 35.453, atomic number 17, is a member of the halogen family (VIIA), and its symbol is “Cl”. Chlorine contains 17 protons and 18 neutrons in is nucleus. There are two isotopes for chlorine as well; Cl-35 and Cl-37. Chlorine was discovered in 1774 by Swedish chemist Carl Wilhelm Sheele. Sheele came upon chlorine when he put a few drops of hydrochloric acid (HCl), then known as muriatic acid, onto a piece of manganese dioxide (MnO2). This caused a reaction where the pricduct was a yellowish-green gas that would later be named chlorine. At this point Sheele thought that this gas contained oxygen and was some sort of oxygen compound,…show more content…
Ferric chloride’s physical state is an orange to brown-black solid. Hydrogen Gold Chloride (HAuCl2) Hydrogen gold chloride is formed again from volcanic reactions. Volcanoes release gases that include steam, carbon dioxide, sulfur dioxide, hydrogen, hydrochloric acid, and hydrogen sulfide. The magma that come from volcanoes contains gold and when this magma and the gases react together, one of the compounds formed is hydrogen gold chloride. The physical state is red crystals. Hydrochloric Acid (HCl) At room temperature hydrochloric acid is a colorless gas. HCl is the compound known as hydrochloric acid, much like H2O is the compound known as water. Hydrochloric acid is produced naturally from the earth, with volcanic eruptions being one outlet. Titanium Tetrachloride (TiCl4) Titanium Tetrachloride is made by a chemical reaction involving titanium dioxide, chlorine gas, and carbon at 1,000 degrees Celsius. When mixed together titanium tetrachloride and carbon dioxide gas are formed. Here is how the reaction looks: TiO2 + 2Cl2 + C ------ TiCl4 + CO2. The physical state of titanium tetrachloride is a yellow liquid. Trichlorosilane (HSiCl3) In the process of getting pure silicon, trichlorosilane is used as an intermediate compound. First silicon must be separated from oxygen where it is found naturally as SiO2. This reaction
Open Document