Phosphorus after this treatment exists as an amorphous network of atoms which reduces strain and gives greater stability, further heating results in the red phosphorus becoming crystalline.
Chronic white phosphorus poisoning of unprotected workers leads to necrosis of the jaw called "phossy-jaw."
White phosphorus (P4) exists as individual molecules, each of which is made up of four phosphorus atoms in a tetrahedral shape.
Phosphorus is a key element in all known forms of life.
The electric furnace method allowed production to increase to the point phosphorus could be used in weapons of war.
Inorganic phosphorus in the form of the phosphate PO43- plays a major role in biological molecules such as DNA and RNA where it forms part of the structural framework of these molecules.
Below is shown a chain of phosphorus atoms which exhibits both the purple and fibrous forms.
Phosphorus is widely distributed in many different minerals.
Ingestion of white phosphorus may cause a medical condition known as "Smoking Stool Syndrome."
Organic compounds of phosphorus form a wide class of materials, some of which are extremely toxic.
Phosphorus was discovered by German alchemist Hennig Brand in 1669 through a preparation from urine, which naturally contains considerable quantities of dissolved phosphates from normal metabolism.
One of the forms of red/black phosphorus is a cubic solid.
Early matches contained white phosphorus, which was dangerous due to its toxicity.
The name phosphorus was derived from the Greek word phosphoros, meaning "light-bearing."
Upon exposure to elemental phosphorus, in the past it was suggested to wash the affected area with two percent copper sulfate solution to form harmless compounds that can be washed away.
The form known as white phosphorus emits a faint glow upon exposure to oxygen.
Phosphorus was first made commercially for the match industry in the nineteenth century.
Samples are commonly coated with white "(di)phosphorus pentoxide," which actually consists of P4O10 molecules.
The allotrope known as red phosphorus does not ignite spontaneously and is far less dangerous.
Red phosphorus does not catch fire in air at temperatures below 240°C, whereas white phosphorus ignites at about 40°C.
An average person contains a little less than 1 kg of phosphorus, about three quarters of which is present in bones and teeth in the form of apatite.
The process involved distilling off phosphorus vapors from precipitated phosphates heated in a retort.
A reaction with oxygen takes place at the surface of the solid (or liquid) phosphorus, forming the short-lived molecules HPO and P2O2 that both emit visible light.
Nevertheless, it should be handled with care because it does revert to white phosphorus in some temperature ranges and, when heated, it emits highly toxic fumes that consist of phosphorus oxides.
A well-fed adult in the industrialized world consumes and excretes about 1-3 g of phosphorus per day in the form of phosphate.
Production of white phosphorus takes place at large facilities and is transported heated in liquid form.
The glucose molecule can exist in an open-chain (acyclic) form and a ring (cyclic) form.
The worst accident in recent times though was an environmental one in 1968 when phosphorus spilled into the sea from a plant at Placentia Bay, Newfoundland.
Just as sulfur forms sulfurous and sulfuric compounds, so phosphorus forms phosphorous and phosphoric compounds.
Elemental phosphorus is then liberated as a vapor and can be collected under phosphoric acid.
When purified artificially, several different allotropic forms of phosphorus can be obtained.
Today phosphorus production is larger than ever, used as a precursor for various chemicals, (Aall 1952).
A recent synthesis of black phosphorus using metal salts as catalysts has been reported.
In 1865, Hittorf discovered that when phosphorus was recrystallized from molten lead, a red/purple form is obtained.
Black phosphorus has an orthorhombic structure (Cmca) and is the least reactive allotrope.
White phosphorus is a yellow, waxy transparent solid.
Burning phosphorus is difficult to extinguish, and if it splashes onto human skin it has horrific effects (see precautions below).
Phosphorus (chemical symbol P, atomic number 15) is a multivalent nonmetal that belongs to the nitrogen group of chemical elements.
Phosphorus can reduce elemental iodine to hydroiodic acid, which is a reagent effective for reducing ephedrine or pseudoephedrine to methamphetamine.
A wide range of organophosphorus compounds are used for their toxicity to certain organisms as pesticides and herbicides, and weaponized as nerve agents.
Red phosphorus may be formed by heating white phosphorus to 250°C (482°F) or by exposing white phosphorus to sunlight.
Each P4O10 molecule has a tetrahedral shape with oxygen inserted between the phosphorus atoms and attached to their vertices.
White phosphorus is insoluble in water but soluble in carbon disulfide.
When a safe process for manufacturing red phosphorus was discovered, with its far lower flammability and toxicity, laws were enacted (under a Berne Convention) requiring its adoption as a safer alternative for match manufacture.
Phosphorus is an essential macromineral, which is studied extensively in soil conservation in order to understand plant uptake from soil systems.
According to the Oxford English Dictionary, the correct spelling of the element is phosphorus.
Nitrogen is used by plants for lots of leaf growth and good green color. Phosphorous is used by plants to help form new roots, make seeds, fruit and flowers. It's also used by plants to help fight disease. Potassium helps plants make strong stems and keep growing fast.
Crops usually display no obvious symptoms of phosphorus deficiency other than a general stunting of the plant during early growth. By the time a visual deficiency is recognized, it may be too late to correct in annual crops. Some crops, such as corn, tend to show an abnormal discoloration when phosphorus is deficient.