Phosphorus is a chemical element with symbol P and atomic number 15. Classified as a nonmetal, Phosphorus is a solid at room temperature. Phosphorus is the chemical element in the periodic table that has the symbol P and atomic number 15. Phosphorus is commonly found in inorganic phosphate rocks and in all living cells. Phosphorus: atom sizes. Atomic radius (empirical): 100 pm Molecular single bond covalent radius: 111 (coordination number 3) ppm; van der Waals radius: 190 ppm; More atomc size properties.

• Phosphorus Atomic Number 15
• Phosphorus Atomic Number And Mass

Phosphorus is a non-metal with diverse biological and industrial significance. It was discovered in 1669 by Hennig Brand and has two allotropic forms and eighteen isotopes.

Discovery and History

The discovery of phosphorus as a novel element was carried out by in Hennig Brand in 1669 by evaporating urine. He obtained a white material that burned brilliantly and emitted a glow in the dark when exposed to oxygen [1]. Antoine Lavoisier identified phosphorus as a separate element in 1777. The name phosphorus also has an interesting origin, as Phosphorus is the name of planet Venus in Ancient Greece language and it means “carrier of light” or “light-bringer”. Commercial scale production of phosphorus was started by Brand and later many scientists, including Robert Boyle, used the same method of phosphorus production developed by Brand. In 1680, Boyle introduced the use of phosphorus to ignite wooden splints with tips of sulfur, and these later were developed into matches [2]. Phosphorus was initially used on a wide scale to make poisons, explosives and nerve agents and due to its toxic and lethal properties, it was commonly named as the “devil’s element”. Gottlieb Gahn and Carl Wilhelm (1796) were the first to discover the presence of phosphorus, in the form of calcium phosphate, in the bones. Until 1840s, one of the major sources of phosphorus has been ashes of bones, and until 1840s. Later in 1850s, the presence of phosphate in rocks on the form of calcium phosphate was discovered and the phosphorus production switched form bones to rocks.

Phosphorus

Occurrence

Phosphorus does not exist in free or elemental state in nature. It forms various compounds and is present in large variety of minerals. The most common source of phosphorus is calcium phosphate that is present in rocks. Phosphorus is an element of great biological value. It is the 6^th most abundant element in the living systems. The largest natural reserves of phosphorus are present in Arab region. Other countries or regions that are significant producers of phosphorus include Russia, China, Florida and Morocco [3]. The annual production of elemental phosphorus is around 1000,000 tons.

Physical Characteristics

White phosphorus is yellowish white solid, that has a waxy texture. Phosphorus undergoes spontaneous ignition in air and forms pentoxide (P₄O₁₀). There are two allotropic forms of phosphorus, red and black, that differ in physical and chemical properties. Red phosphorus (which is formed by heating of white phosphorus at high temperature) ignites on friction. White phosphorus is a highly toxic substance., while red phosphorus is non-toxic [4]. Phosphorus is water insoluble. Black phosphorus is also termed as violet phosphorus and is the least reactive allotrope of phosphorus. It resembles graphite in appearance and structure.

Chemical Characteristics

White phosphorus is very reactive element. In the presence of oxygen, white phosphorus emits a light green glow, termed as chemiluminescence (glow caused by cold chemical reaction) [5]. The most abundant compounds of phosphorus contain the tetrahedral anion of phosphate (PO₄^3-). There is a vast variety of phosphorus compounds including oxoacids (phosphoric acid), sulfides, nitrides (phosphorus nitride halogens (F2PN, Cl2PN), and phosphides (reaction of metals with red phosphorus). Phosphine (PH3) is a toxic compound with pungent smell, is structural analogue of ammonia. Diphosphine (P2H4), is an analogue of hydrazine and is highly flammable.

Uses and Significance

• The largest use of phosphorus is in the production of fertilizers. It is an essential nutrient for the growth of plants.
• Phosphorus is used in making of safety matches, and various ammunitions, such as incendiary shells and hand grenades etc.
• Phosphorus is used in the manufacturing of bronze and steel.
• It is used in making LEDs (light-emitting diodes).
• Phosphorus is used in making detergents, that functions to remove water hardness and improve the efficiency of detergent.
• It is used in synthesis of nerve agents.
• It is used as active ingredient in various pesticides.
• Phosphoric acid is widely used in manufacturing of soft drinks, baking powder.
• Various compounds of phosphate are used in processing of cheese and meat.

Health Hazards

Phosphorus in the form of phosphate is a vital compound for all living systems. The energy currency of cell, ATP (adenosine triphosphate) that regulates every process in the living cell, uses phosphate. Phosphorylation, that is the process of adding phosphate to various biological molecules, is an important regulatory mechanism in living organisms. Lipids in combination with phosphorus (phospholipids) are the primary building blocks of cell membrane. Phosphorus is present in the building blocks of RNA and DNA. A balanced diet includes a definitive everyday intake of phosphorus. About 0.7 kg of phosphorus is present in an average adult human being, mostly in teeth and bones and in soft tissues of the body. deficiency of phosphate in the body can lead to various physiological effects, including tissue weakness, neurological defects and lack of ATP. Increased intake of phosphate can cause hardening of tissues and organs and diarrhea.

Phosphorus Atomic Number 15

Isotopes of Phosphorus

There are twenty-three isotopes of phosphorus, that range in atomic numbers from 26 to 43. Natural phosphorus constitutes only one stable isotope, phosphorus-31 [6].

Phosphorus Atomic Number And Mass

REFERENCES

[1]. Beatty, Richard (2000). Phosphorus. Marshall Cavendish. p. 7. ISBN0-7614-0946-7.

[2]. Peter Baccini; Paul H. Brunner. Metabolism of the Anthroposphere. MIT Press, 2012. p. 288. ISBN0262300540.

[3]. Philpott, Tom (March–April 2013). “You Need Phosphorus to Live—and We’re Running Out”. Mother Jones.fwhi

[4]. Abundance. ptable.com

[5]. Michael A. Sommers. Phosphorus. The Rosen Publishing Group, 2007. p. 25. ISBN1404219609.

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