Phosphorus

Phosphorus, ₁₅P
	Forms of phosphorus Waxy white Light red Dark red and violet Black waxy white (yellow cut), red (granules centre left, chunk centre right), and violet phosphorus
Phosphorus
Pronunciation	/ˈfɒsfərəs/ (FOS-fər-əs)
Allotropes	white, red, violet, black and others (see Allotropes of phosphorus)
Appearance	white, red and violet are waxy, black is metallic-looking
Standard atomic weight Ar°(P)
	30.973761998(5)
Abundance
in the Earth's crust	5.2 (silicon = 100)
Phosphorus in the periodic table
	silicon ← phosphorus → sulfur
Atomic number (Z)	15
Group	group 15 (pnictogens)
Period	period 3
Block	p-block
Electron configuration	[Ne] 3s2 3p3
Electrons per shell	2, 8, 5
Physical properties
Phase at STP	solid
Melting point	white: 317.3 K (44.15 °C, 111.5 °F) ; red: ∼860 K (∼590 °C, ∼1090 °F)
Boiling point	white: 553.7 K (280.5 °C, 536.9 °F)
Sublimation point	red: ≈689.2–863 K (≈416–590 °C, ≈780.8–1094 °F) ; violet: 893 K (620 °C, 1148 °F)
Density (near r.t.)	white: 1.823 g/cm3; red: ≈2.2–2.34 g/cm3 ; violet: 2.36 g/cm3 ; black: 2.69 g/cm3
Heat of fusion	white: 0.66 kJ/mol
Heat of vaporization	white: 51.9 kJ/mol
Molar heat capacity	white: 23.824 J/(mol·K)
Atomic properties
Oxidation states	−3, −2, −1, 0, +1, +2, +3, +4, +5 (a mildly acidic oxide)
Electronegativity	Pauling scale: 2.19
Ionization energies	1st: 1011.8 kJ/mol ; 2nd: 1907 kJ/mol ; 3rd: 2914.1 kJ/mol ; (more) ;
Covalent radius	107±3 pm
Van der Waals radius	180 pm
	Spectral lines of phosphorus
Other properties
Natural occurrence	primordial
Crystal structure	body-centered cubic (bcc)
Thermal conductivity	white: 0.236 W/(m⋅K) ; black: 12.1 W/(m⋅K)
Magnetic ordering	white, red, violet, black: diamagnetic
Molar magnetic susceptibility	−20.8×10−6 cm3/mol (293 K)
Bulk modulus	white: 5 GPa; red: 11 GPa
CAS Number	7723-14-0 (red); 12185-10-3 (white)
History
Discovery	Hennig Brand (1669)
Recognised as an element by	Antoine Lavoisier (1777)
Isotopes of phosphorus v; e;
	Category: Phosphorus; view; talk; edit; \| references

Phosphorus has the chemical symbol P, and its atomic number is 15. Its mass number is 30.97. It is not found in nature as an element, but as compounds, such as phosphates. There are many different forms. The most common form is a red or white waxy solid.

Properties

Physical properties

Phosphorus comes in several forms. White and red phosphorus are the most common forms. White phosphorus is a waxy white solid. When pure, it is colourless. It is insoluble in water, but soluble in carbon disulfide, an organic solvent. It turns light yellow when in air. It glows in the dark because it "burns" very slowly in air.

When exposed to sunlight, or when heated in its own vapour to 250 °C, it is converted to the red variety. This form does not ignite spontaneously and it is less toxic and less flammable than white phosphorus. The red modification is fairly stable and sublimes with a vapor pressure of 1 atmosphere at 417 °C.

Chemical properties

White phosphorus is more reactive than red phosphorus. White phosphorus catches fire spontaneously in air, burning to make smoke of phosphorus(V) oxide. If it burns in a little air, it produces poisonous phosphorus(III) oxide. When white phosphorus is heated in an alkali, it disproportionates to produce hypophosphites and phosphine. Red phosphorus can burn but needs to be ignited. Phosphorus reacts with the halogens to make phosphorus halides. It reacts with some metals to make phosphides.

Chemical compounds

Phosphorus compounds are chemical compounds containing phosphorus. They are listed below with some of their properties. Phosphorus comes in several oxidation states, the number of electrons moved during a redox reaction. -3 is flammable, powerful reducing agent, and toxic; +1 is a strong reducing agent and is rare; +3 is a weaker reducing agent that is poisonous; +5 is not a reducing agent and is very common.

In -3 oxidation state

Phosphides

Phosphine, toxic gas that smells like fish and ignites by itself
Phosphide, the ion
Sodium phosphide

Other compounds

Phosphonium, another ion

In +1 oxidation state

Hypophosphorous acid, salts are called hypophosphites
Sodium hypophosphite

In +3 oxidation state

Phosphites

Phosphorous acid, poisonous, salts are called phosphites
Sodium phosphite

Other compounds

Phosphorus trichloride
Phosphorus triiodide
Phosphorus(III) oxide, phosphorus trioxide, poisonous, garlic-smelling

In +5 oxidation state

Phosphates

Phosphoric acid, most common, salts are called phosphates
Calcium phosphate
Dicalcium phosphate
Monocalcium phosphate
Sodium phosphate
Zinc phosphate

Other compounds

Phosphorus(V) oxide, phosphorus pentoxide, absorbs water
Phosphorus(V) chloride

Phosphoric acid
Trisodium phosphate
Phosphorus pentachloride (left) and phosphorus trichloride (right)

Occurrence

It is an essential component of living systems and is found as phosphate in nervous tissue, bones and cell protoplasm. It is also found in the earth as phosphate rock. Phosphate rock is the main source of phosphorus and phosphorus compounds. Many body tissues have calcium phosphates in them.

Preparation

Phosphorus was first made by heating a mixture of phosphates and carbon in an iron pot. The phosphates were made by dissolving bones in strong acids and evaporating the solution.

Phosphorus is made now by heating calcium phosphate, carbon, and silicon dioxide in an electric arc furnace. The heat of the electric arc melts the mixture of materials, and phosphorus gas is given off. It is absorbed under water. This makes white phosphorus.

Uses

As an element

White phosphorus is used in incendiary weapons and smoke grenades. It is also used to make organic compounds that have phosphorus in them. Phosphorus is used to dope semiconductors. Phosphorus is used to remove oxygen from copper. It is also used in making alloys. Red phosphorus is used in matches and flares.

As chemical compounds

Phosphorus compounds are used for fertilizers, soft drinks, toothpaste, and detergents. Most of these are phosphates. Phosphides can be used to kill rodents.

Safety

White phosphorus is very dangerous. It is very toxic and ignites easily, burning with a very hot flame. Red phosphorus is much safer. Some phosphorus compounds are toxic, but the common phosphates are not toxic.

Related pages

↑ "Standard Atomic Weights: Phosphorus". CIAAW. 2013.
↑ "Phosphorus: Chemical Element". Encyclopædia Britannica.
↑ Wang, Yuzhong; Xie, Yaoming; Wei, Pingrong; King, R. Bruce; Schaefer, Iii; Schleyer, Paul v. R.; Robinson, Gregory H. (2008). "Carbene-Stabilized Diphosphorus". Journal of the American Chemical Society. 130 (45): 14970–1. doi:10.1021/ja807828t. PMID 18937460.
↑ Ellis, Bobby D.; MacDonald, Charles L. B. (2006). "Phosphorus(I) Iodide: A Versatile Metathesis Reagent for the Synthesis of Low Oxidation State Phosphorus Compounds". Inorganic Chemistry. 45 (17): 6864–74. doi:10.1021/ic060186o. PMID 16903744.
↑ Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". CRC Handbook of Chemistry and Physics (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
↑ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
↑ cf. "Memoir on Combustion in General" Mémoires de l'Académie Royale des Sciences 1777, 592–600. from Henry Marshall Leicester and Herbert S. Klickstein, A Source Book in Chemistry 1400–1900 (New York: McGraw Hill, 1952)

[1] "Standard Atomic Weights: Phosphorus". CIAAW. 2013.

[2] "Phosphorus: Chemical Element". Encyclopædia Britannica.

[3] Wang, Yuzhong; Xie, Yaoming; Wei, Pingrong; King, R. Bruce; Schaefer, Iii; Schleyer, Paul v. R.; Robinson, Gregory H. (2008). "Carbene-Stabilized Diphosphorus". Journal of the American Chemical Society. 130 (45): 14970–1. doi:10.1021/ja807828t. PMID 18937460.

[4] Ellis, Bobby D.; MacDonald, Charles L. B. (2006). "Phosphorus(I) Iodide: A Versatile Metathesis Reagent for the Synthesis of Low Oxidation State Phosphorus Compounds". Inorganic Chemistry. 45 (17): 6864–74. doi:10.1021/ic060186o. PMID 16903744.

[5] Lide, D. R., ed. (2005). "Magnetic susceptibility of the elements and inorganic compounds". CRC Handbook of Chemistry and Physics (PDF) (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.

[6] Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.

[7] . "Memoir on Combustion in General" Mémoires de l'Académie Royale des Sciences 1777, 592–600. from Henry Marshall Leicester and Herbert S. Klickstein, A Source Book in Chemistry 1400–1900 (New York: McGraw Hill, 1952)

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