Got Any info on Phosphorus?
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Phosphorus, (IPA: /ˈfɒsfərəs/, Greek: phôs meaning "light", and phoros meaning "bearer"), is the chemical element in the periodic table that has the symbol P and atomic number 15. A multivalent nonmetal of the nitrogen group, phosphorus is commonly found in inorganic phosphate rocks and in all living cells.\n\nPhosphorus exists in several allotropes, most commonly white, red and black. White phosphorus (P4) contains only four atoms, resulting in very high ring strain and instability. White phosphorus glows in the dark, is highly flammable and pyrophoric (self-igniting) upon contact with air as well as toxic. Red phosphorus has a network form which reduces strain and gives greater stability. Red phosphorus does not catch fire in air at temperatures below 240°C whereas white phosphorus ignites at about 40°C. Black phosphorus is amorphous and is the least reactive allotrope.\n\nRed phosphorus is formed by heating white phosphorus to 250°C (482°F) or by exposing white phosphorus to sunlight.\n\nDue to its high reactivity, phosphorus is never found as a free element in nature. It emits a faint glow upon exposure to oxygen (hence its Greek derivation and the Latin meaning 'morning star') and is an essential element for living organisms. The most important commercial use of phosphorus-based chemicals is the production of fertilizers. They are also widely used in explosives, nerve agents, friction matches, fireworks, pesticides, toothpaste, and detergents.\n\nContents [hide]\n1 Characteristics \n1.1 Glow \n2 Applications \n3 Biological role \n4 History \n5 Occurrence \n6 Precautions \n7 Isotopes \n8 Spelling \n9 Compounds \n10 References \n11 External links \n \n\n\n[edit] Characteristics\nPhosphorus, in its common form, is a waxy white (or yellowish) solid that has a characteristic, disagreeable smell similar to that of garlic. Pure forms of the element are colorless and transparent. This nonmetal is not soluble in water, but is soluble in carbon disulfide. The white allotrope ignites spontaneously in air; however both white and red phosphorus burn in air to produce phosphorus pentoxide.\n\n\n[edit] Glow\nThe glow from phosphorus was the attraction of its discovery around 1669, but the mechanism for that glow was not fully described until 1974.[1] It was known from early times that the glow would persist for a time in a stoppered jar but then cease. Robert Boyle in the 1680s ascribed it to "debilitation" of the air. In fact it is oxygen being consumed. By the 18th century it was known that in pure oxygen phosphorus does not glow at all,[2] there is only a range of partial pressure where it does, too high or too low and the reaction stops. Heat can be applied to drive the reaction at higher pressures.[3]\n\nIn 1974 the glow was explained by R. J. van Zee and A. U. Khan.[1] A reaction with oxygen takes place at the surface of the solid (or liquid) phosphorus, forming short-lived molecules HPO and P2O2 and they both emit visible light. The reaction is slow and only very little of the intermediates is required to produce the luminescence, hence the extended time the glow continues in a stoppered jar.\n\nAlthough the term phosphorescence is derived from phosphorus, the reaction is properly called luminescence (glowing by its own reaction, in this case chemoluminescence), not phosphorescence (re-emitting light that previously fell on it).\n\n\n[edit] Applications\nConcentrated phosphoric acids, which can consist of 70% to 75% P2O5 are very important to agriculture and farm production in the form of fertilizers. Global demand for fertilizers led to large increases in phosphate (PO43-) production in the second half of the 20th century. Other uses;\n\nPhosphates are utilized in the making of special glasses that are used for sodium lamps. \nBone-ash, calcium phosphate, is used in the production of fine china. \nSodium tripolyphosphate made from phosphoric acid is used in laundry detergents in sev
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If you are really interested in this topic, I recommend reading "The Plutonium Files," a recently published book. It reports on the negative health effects of uranium and plutonium, specifically the results of secret tests performed on civilian citizens and members of the military, by our government. (Almost all of whom were unaware they had unwittingly become guinea pigs.) Very interesting and informative.
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go the government food puyramid website\nvery informational and useful
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IAnd for your other request, I would request you to send a seperate mail to me through yahoo Answer so that I am able to send it part by part.These are long subjects and would take some time,The balanced equation would be                                           H3PO4+3KOH=K3PO4+3H2O
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N(Nitrogen), P(Phosphorus), K(Potassium)
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phosphorescence, this link should tell you.
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See this link\n\nhttp://us.badm.washington.edu/yalch/Research/atmosphe.htm
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http://en.wikipedia.org/wiki/Calcium
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In agriculture phosphate refers to one of the three primary plant nutrients, and it is a component of fertilizers. Rock phosphate is quarried from phosphate beds in sedimentary rocks. In former times it was simply crushed and used as is, but the crude form is now used only in organic farming. Normally it is chemically treated to make superphosphate, triple superphosphate, or ammonium phosphates, which have higher concentration of phosphate and are also more soluble, therefore more quickly usable by plants.
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You can use either phosphoric acid solution (35%) or tannic acid solution (20%). Phosphates give a grey/black. Tannate gives a BLUE/BLACK. If you are trying to "parkerise" the surface there are a number of commercial parkerizing solutions available.
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Agricultural Applications - radioactive tracers\n\n\nRadioisotopes can be used to help understand chemical and biological processes in plants. This is true for two reasons: 1)radioisotopes are chemically identical with other isotopes of the same element and will be substituted in chemical reactions and 2)radioactive forms of the element can be easily detected with a Geiger counter or other such device.\nExample:\nA solution of phosphate, containing radioactive phosphorus-32, is injected into the root system of a plant. Since phosphorus-32 behaves indentically to that of phosphorus-31, the more common and non-radioactive form of the element, it is used by the plant in the same way. A Geiger counter is then used to detect the movement of the radioactive phosphorus-32 throughout the plant. This information helps scientists understand the detailed mechanism of how plants utilized phosphorus to grow and reproduce.
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http://en.wikipedia.org/wiki/PH
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temp 30-34 deg C\nadequate Nitrogen & Phosphorus\nwell watered but well drained\nNot too Humid\nC02 level 1000ppm
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Hi, check this site out.  It has the most detailed nutritional information I have ever seen.  Should be exactly what your looking for.  Hope this helps.
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phosphates, potash, shale oil
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Try Wikipedia.org...Qualitative inorganic analysis. I was just there.
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Take the Homeopathic Remedy SULFUR in 200 potency just once a day first thing in the morning for three days in a row stop for one day and if you are not any better take it for three more days. If the problem still persists take PHOSPHORUS 200 once daily half our before going to bed for a week No side effects and No Complications.\nTake care and God Bless you !