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Out of the four stable halogens, only fluorine and chlorine have reduction potentials higher than that of oxygen, allowing them to form hydrofluoric acid and hydrochloric acid directly through reaction with water. [17] The reaction of fluorine with water is especially hazardous, as an addition of fluorine gas to cold water will produce ...
Burning lithium metal produces lithium oxide. Lithium oxide forms along with small amounts of lithium peroxide when lithium metal is burned in the air and combines with oxygen at temperatures above 100 °C: [3] 4Li + O 2 → 2 Li 2 O. Pure Li 2 O can be produced by the thermal decomposition of lithium peroxide, Li 2 O 2, at 450 °C [3] [2] 2 Li ...
The most reactive metals, such as sodium, will react with cold water to produce hydrogen and the metal hydroxide: 2 Na (s) + 2 H 2 O (l) →2 NaOH (aq) + H 2 (g) Metals in the middle of the reactivity series, such as iron , will react with acids such as sulfuric acid (but not water at normal temperatures) to give hydrogen and a metal salt ...
Lithium will ignite and burn in oxygen when exposed to water or water vapor. In moist air, lithium rapidly tarnishes to form a black coating of lithium hydroxide (LiOH and LiOH·H 2 O), lithium nitride (Li 3 N) and lithium carbonate (Li 2 CO 3, the result of a secondary reaction between LiOH and CO 2). [48] Lithium is one of the few metals that ...
This reaction initially produces lithium hydroperoxide: [4] [5] LiOH + H 2 O 2 → LiOOH + H 2 O. This lithium hydroperoxide may exist as lithium peroxide monoperoxohydrate trihydrate (Li 2 O 2 ·H 2 O 2 ·3H 2 O). Dehydration of this material gives the anhydrous peroxide salt: 2 LiOOH → Li 2 O 2 + H 2 O 2. Li 2 O 2 decomposes at about 450 ...
With water-containing acids, LiH reacts faster than with water. [3]: 8 Many reactions of LiH with oxygen-containing species yield LiOH, which in turn irreversibly reacts with LiH at temperatures above 300 °C: [3]: 10 LiH + LiOH → Li 2 O + H 2. Lithium hydride is rather unreactive at moderate temperatures with O 2 or Cl 2.
At higher (but still cryogenic) temperatures, lithium superoxide can be produced by ozonating lithium peroxide (Li 2 O 2) in freon 12: Li 2 O 2 (f 12) + 2 O 3 (g) → 2 LiO 2 (f 12) + 2 O 2 (g) The resulting product is only stable up to −35 °C. [5] Alternatively, lithium electride dissolved in anhydrous ammonia will reduce oxygen gas to ...
The lithium–air battery (Li–air) is a metal–air electrochemical cell or battery chemistry that uses oxidation of lithium at the anode and reduction of oxygen at the cathode to induce a current flow. [1] Pairing lithium and ambient oxygen can theoretically lead to electrochemical cells with the highest possible specific energy.