Chapters: Ammonium Perchlorate, Perchloric Acid, Potassium Perchlorate, Sodium Perchlorate, Lithium Perchlorate, Caesium Perchlorate, Silver Perchlorate, Fluorine Perchlorate, Nitronium Perchlorate, Magnesium Perchlorate, Rubidium Perchlorate. Source: Wikipedia. Pages: 56. Not illustrated. Free updates online. Purchase includes a free trial membership in the publisher's book club where you can select from more than a million books without charge. Excerpt: Perchlorates are the salts derived from perchloric acid (HClO4). They occur both naturally and through manufacturing. They have been used as a medicine for more than 50 years to treat thyroid gland disorders. They are used extensively within the pyrotechnics industry, and ammonium perchlorate is also a component of solid rocket fuel. Lithium perchlorate, which decomposes exothermically to give oxygen, is used in oxygen "candles" on spacecraft, submarines and in other esoteric situations where a reliable backup or supplementary oxygen supply is needed. Most perchlorate salts are soluble in water. The chemical notation for the perchlorate ion is . The ion has a molecular mass of 99.45 amu. A perchlorate (compound) is a compound containing this group, with chlorine in oxidation state +7. The perchlorate ion is the least reactive oxidizer of the generalized chlorates. This is apparently paradoxical, since higher oxidation numbers are expected to be progressively stronger oxidizers, and less stable. Perchlorate does in fact have the highest redox potential and is least stable thermodynamically, but the central chlorine is a closed shell atom and well protected by the four oxygens. Hence, perchlorate reacts sluggishly. Most perchlorate compounds, especially salts of electropositive metals such as sodium perchlorate or potassium perchlorate, are slow to react unless heated. This property is useful in many applications, such as flares, where the device should not explode, or even c...More: http: //booksllc.net/?id=61117