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Phosphides arise by reaction of metals with red phosphorus. The alkali metals (group 1) and alkaline earth metals can form ionic compounds containing the phosphide ion, P 3−. These compounds react with water to form phosphine. Other phosphides, for example Na 3 P 7, are known for these reactive metals.
Red phosphorus can also be used in the illicit production of methamphetamine and Krokodil. Red phosphorus can be used as an elemental photocatalyst for hydrogen formation from the water. [13] They display a steady hydrogen evolution rates of 633 μmol/(h⋅g) by the formation of small-sized fibrous phosphorus. [14]
Water-reactive substances [1] are those that spontaneously undergo a chemical reaction with water, often noted as generating flammable gas. [2] Some are highly reducing in nature. [ 3 ] Notable examples include alkali metals , lithium through caesium , and alkaline earth metals , magnesium through barium .
Higher temperature or acidic conditions can speed up the hydrolysis reactions considerably. [5] Conversely, polyphosphoric acids or polyphosphates are often formed by dehydrating a phosphoric acid solution; in other words, removing water from it often by heating and evaporating the water off.
PCl 3 reacts vigorously with water to form phosphorous acid (H 3 PO 3) and hydrochloric acid: PCl 3 + 3 H 2 O → H 3 PO 3 + 3 HCl. Phosphorus trichloride is the precursor to organophosphorus compounds. It reacts with phenol to give triphenyl phosphite: 3 PhOH + PCl 3 → P(OPh) 3 + 3 HCl (Ph = C 6 H 5)
The noble gases do not react with water, but their solubility in water increases when going down the group. Argon atoms in water appear to have a first hydration shell composed of 16±2 water molecules at a distance of 280–540 pm, and a weaker second hydration shell is found out to 800 pm. Similar hydration spheres have been found for krypton ...
Elemental phosphorus is distilled out of the furnace and burned with air to produce high-purity phosphorus pentoxide, which is dissolved in water to make phosphoric acid. [22] The thermal process produces phosphoric acid with a very high concentration of P 2 O 5 (about 85%) and a low level of impurities.
White phosphorus, yellow phosphorus, or simply tetraphosphorus (P 4) is an allotrope of phosphorus. It is a translucent waxy solid that quickly yellows in light (due to its photochemical conversion into red phosphorus ), [ 2 ] and impure white phosphorus is for this reason called yellow phosphorus.