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PhosphorusFrom Wikipedia, the free encyclopedia

This article is about the chemical element. For other uses, seePhosphorus (disambiguation).

silicon phosphorus sulfur

N

P

As

15PPeriodic table

Appearance

colorless, waxy white, yellow, scarlet, red, violet, black

waxy white (yellow cut), red, violet and black phosphorus

General properties

Name, symbol,number phosphorus, P, 15

Element category nonmetal

Group, period,block 15, 3,p

Standard atomic weight 30.973762(2)gmol1

Electron configuration [Ne] 3s2

3p3

Electrons pershell 2, 8, 5 (Image)

Physical properties

Density(near r.t.) (white) 1.823, (red) 2.2 2.34, (violet) 2.36, (black)

2.69 gcm3

Melting point (white) 44.2 C, (black) 610 C

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Subli

i

i

(red) 416 590 C (vi let) 620 C

B

ili

i

(white) 280.5 C

H

usi (white) 0.66 kJmol

1

H

v

iz

i (white) 12.4 kJmol

1

Speci

ic heat capacity (25 C) (white)

23.824 Jmol 1

K1

Vapor pressure (white)

P/Pa 1 10 100 1 k 10 k 100 k

atT/K 279 307 342 388 453 549

Vapor pressure (red, bp. 431 C)

P/Pa 1 10 100 1 k 10 k 100 k

atT/K 455 489 529 576 635 704

Atomic properties

Oxidation states

5, 4, 3, 2[1]

, 1[2]

, -1, -2, -3(mildl acidic oxide)

Electronegativity 2.19 (Pauli scale)

Ionization energies

(more)

1st: 1011.8 kJmol1

2nd: 1907 kJmol1

3rd: 2914.1 kJmol1

Covalent radius 107

3 pm

Van der Waals radius 180 pm

Miscellanea

Magnetic ordering

(white,red,violet,black) diamagnetic[3]

Thermal conductivity (300 K) (white) 0.236, (black) 12.1 Wm1

K1

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Bul

modulus

(white) 5, (red) 11 GPa

CAS registry number 7723-14-0

Most stable isotopes

Main article:Isotopes of phosphorus

iso NA hal

-li

e DM DE(MeV) DP

31P 100%

31Pis stable with 16 neutrons

32P syn 14.28 d

1.709

32S

33

P syn

25.3 d

0.24933

S

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Contents

[hide]

1 Physical properties

o 1.1 Glow from white phosphorus

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o 1.2 Allotropes

o 1.3 Isotopes

2 Chemical properties

o 2.1 Chemicalbonding

o 2.2 Phosphine, diphosphine and phosphonium salts

o 2.3 Halides

o 2.4 Oxides and oxyacids

3 Spellingand etymology

4 History and discovery

5 Occurrence

6 Production

7 Applications

8 Biological role

9 Precautions

o 9.1 US DEA List I status

10 See also

11 Notes

12 References

o 12.1 Notes

o 12.2 Sources

13 Externallinks

[edit]P i l erties

[edit]Glow from white phosphorus

Id

1669, Germanale

f

emist Hennig Brandtattempted tgdistil some

h

indof "lifeessence" fromf

is

irine, and in t

f

eprocessf

eproduceda wf

itematerial tf

at glowed in tf

edark.[4]

Tf

ephosphorushad

in fact beenproduced from inorganicphosphate, which isasignificant component ofdissolvedurine

solids.p

hitephosphorus ishighlqreactiveand givesoffa faint greenish glow uponuniting

withoxqgen. The glow observed b

qBrand wasactuall

qcaused b

qthe veryslow burning of the

phosphorus, but asheneithersaw flamenorfelt anyheat hedidnot recognize it as burning.

It wasknown fromearly times that the glow wouldpersist fora time inastoppered jarbut then

cease. Robert Boyle in the 1680sascribed it to "debilitation" of theair; in fact, it isoxygen being

consumed. By the 18thcentury, it wasknown that inpureoxygen, phosphorusdoesnot glow at

all;[5]

there isonlyarangeofpartial pressureat which it does. Heat can beapplied todrive the

reactionat higherpressures.[6]

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Inr

s

74, thetlo

u

uas e

vplained

wy

x

. J.yan Zee and A. U. Khan.

[7]A reaction

uith o

vy

ten takes

place at the surface of the solid

or liquid) phosphorus, formint

the shortli

yed molecules

PO and

P2O2 that w oth emit y isi w le li t ht.

he reaction is slou

and onlyyery little of the intermediates are

required to produce the luminescence, hence the evtended time the

tlo

ucontinues in a stoppered jar.

Althout h the term phosphorescence is deri y ed from phosphorus, the reaction u hich t i y es

phosphorus itst

lou

is properly called chemiluminescence

tlo

uin

tdue to a cold chemical reaction),

not phosphorescence

reemittin

tli

tht that pre

yiously fell onto a su

wstance and e

vcited it).

Phosphorescence is the slou

decay of a metastaw

le electronic state to a lou

er enerty state throu

th

emission of lit

ht.

he decay is slou

w

ecause the transition from the evcited to the lo

uer state requires

a spin flip, makint

it classicallyforw

idden. Often it inyol

yes a transition from an e

vcited triplet state to

a sint

lett

round state.

he metastaw

le evcited state may ha

ye

ween populated

wy thermal e

vcitations

or some li t ht source. Since phosphorescence is slo u , it persists for some time after the e v citint

source is remo y ed. In contrast, chemiluminescence occurs u hen the product molecules of a chemical

reaction

PO and P2O2 in this case) lea y e the reaction in an electronically e v cited state.

hese

evcited molecules then release their e

vcess ener

ty in the form of li

tht.

he frequency

colour) of the

lit

ht emitted is proportional to the enert

y difference of the tu

o electronic states inyol

yed.

[8]

[edit]Allotropes

Main article:Allotropes ofphosphorus

P4 molecule

Phosphorus has se

eral formsallotropes)

hich ha

e strikinly different properties.

[9]

he t

o most

common allotropes arewhitephosphorus and redphosphorus.

ed phosphorus is an intermediate

phaseet

een

hite and

iolet phosphorus. Another form, scarlet phosphorus, is o

tained

y

allo

in

a solution of

hite phosphorus incaron disulfide to e

aporate in sunli

ht. Black phosphorus

is o

tained

y heatin

hite phosphorus under hi

h pressures

a

out2,

atmospheres). In

appearance, properties, and structure, it resem

les

raphite,

ein

lack and flaky, a conductor of

electricity, and has puckered sheets of linked atoms. Another allotrope isdiphosphorus; it contains a

phosphorus dimeras a structural unit and is hi

hly reactie.

[10]

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P4O10 molecule

Whitephosphorushas t o forms, lo temperature form and hi

htemperature form.

heyoth

contain a phosphorus P4tetrahedron as a structural unit, in hich each atom is ound to the other

three atoms y a sin

le ond.

his P4 tetrahedron is also present in liquid and

aseous phosphorus

up to the temperature of800 C

hen it starts decomposin

to P2molecules.[11]

White phosphorus is

the least sta

le, the most reactie, more

olatile, lessdense, and more to

ic than the other allotropes.

he toicity of

hite phosphorus led to its discontinued use in matches. White phosphorus is

thermodynamically unsta

le at normal condition and

ill

radually chan

e to red phosphorus.

his

transformation, hich is accelerated y li

ht and heat, makes hite phosphorus almost al ays

contain some red phosphorus and therefore appear yello . For this reason, it is also called yello

phosphorus. It

lo

s

reenish in the dark

hen eposed to o

y

en), is

hi

hly flammale and pyrophoric

self

i

nitin

) upon contact

ith air as

ell as toic

causin

seere

li er dama

e on in

estion). Because of pyrophoricity, hite phosphorus is used as an additi e

in napalm.

he odour of com

ustion of this form has a characteristic

arlic smell, and samples are

commonly coated

ith

hite

di)phosphorus pentoide

,

hich consists of P4O10 tetrahedra ith

oy

en inserted

et

een the phosphorus atoms and at theirertices. White phosphorus is insolu

le

in

ater

ut solu

le in caron disulfide.

[12]

he

hite allotrope can

e produced usin

se

eral different methods. In one

process, calcium phosphate,

hich is deried from phosphate rock, is heated in an electric or fuel

fired furnace in the presence ofcar

on and silica.[13]

Elemental phosphorus is then li

erated as a

apour and can

e collected underphosphoric acid.

his process is similar to the first synthesis of

phosphorus from calcium phosphate inurine.

Crystal structure of red phosphorus

In the redphosphorus, one of the P4 onds is roken, and one additional ond is formed ith a

nei

h

ourin

tetrahedron resultin

in a more chain

like structure.j

ed phosphorus may

e formed

yheatin

hite phosphorus to 2k

0 C482 F) or

y e

posin

hite phosphorus to

sunli

ht.[4]

Phosphorus after this treatment eists as an amorphous net

ork of atoms

hich reduces

strain and

i

es

reater sta

ility; further heatin

results in the red phosphorus

ecomin

crystalline.

herefore red phosphorus is not a certain allotrope,

ut rather an intermediate phase

et

een the

hite and

iolet phosphorus, and most of its properties ha

e a ran

e ofalues.

jed phosphorus does

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not catch fire in air at temperaturesl

elom

2n0C,

mhereas

mhite phosphorus i

onites at a

lout

30 C.[14]

Violetphosphorus is a thermodynamic sta l le form of phosphorus m hich can l e produced l y day

lon o temper of red phosphorus a l o e 0 C. In 1865,

ittorfdisco ered that m hen phosphorus m as

recrystalli ed from molten lead, a red/purple form is o l tained. herefore this form is sometimes knom n

as

ittorf's phosphorus

oriolet or metallic phosphorus).

[10]

Crystal structure of

lack phosphorus

Blackphosphorus is the least reacti e allotrope and the thermodynamic sta l le form l elo m 550 C. It

is also knom

n as metallic phosphorus and has a structure somem

hat reseml

lino

that

ofo

raphite.[15][16]

io

h pressures are usually required to producel

lack phosphorus,l

ut it can alsol

e

produced at aml

ient conditions usino

metal salts as catalysts.[17]

he diphosphorus allotrope, P2, is stal le only at hi o h temperatures. he dimeric unit contains a triple

l ond and is analo o ous to 2. he diphosphorus allotrope

P2) can l e o l tained normally only under

ez

treme conditions

for ez

ample, from P4 at 1100 kel in). e ertheless, some ad ancements m ere

ol

tained ino

eneratino

the diatomic molecule in homoo

eneous solution, under normal conditionsm

ith

the usel

y some transitional metal complez

es

lased on, for e

z

ample,tuno

sten and niol

ium).[18]

Properties of some allotropes of phosphorus[9][10]

Form white() white(){

iolet black

Symmetry Body-centred cubic Triclinic Monoclinic Orthorhombic

Pearson symbol

aP24 mP84 oS8

Space group I-43m P-1 No.2 P2/c No.13 Cmca No.64

Density (g/cm3) 1.828 1.88 2.36 2.69

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Bandgap (eV) 2.1 1.5 0.34

Refractive index 1.8244 2.6 2.4

[edit]IsotopesMai

|

article: Isotopesofphosphorus

Although twenty-three isotopesofphosphorusareknown[19]

(all possibilities from}

4P up to

46P),

only31

P, withspin 1/~

, isstableand is thereforepresent at 100% abundance. Thehalf-integerspin

andhighabundanceof31

P make it useful fornuclearmagneticresonancestudiesof biomolecules,

particularly DNA.

Tworadioactive isotopesofphosphorushavehalf-lives whichmake themuseful forscientific

experiments.3

}

P hasahalf-lifeof 14.~

6~

daysand33

P hasahalf-lifeof~

5.34days. Biomoleculescan

be "tagged" witharadioisotope toallow forthestudyof verydilutesamples.

Radioactiveisotopesofphosphorus include

3

P, abeta-emitter (1.1 MeV) withahalf-lifeof 14.3 days which isusedroutinely in life-science

laboratories, primarily toproduceradiolabeled DNA and RNA probes, e.

. foruse inNorthern

blotsorSouthern blots. Because thehighenergy betaparticlesproducedpenetrateskin

andcorneas, and becauseany3

P ingested, inhaled, orabsorbed isreadily incorporated into

boneandnucleicacids,

ccupational Safetyand Health Administration in the

nited States, and

similarinstitutions inotherdevelopedcountriesrequire that alab coat, disposable gloves,

andsafety glassesorgoggles be worn when working with3

P, and that working directlyoveranopencontainerbeavoided inordertoprotect theeyes.Monitoringpersonal, clothing, andsurface

contamination isalsorequired. Inaddition, due to thehighenergyof the beta

particles, shielding thisradiation with thenormallyuseddensematerials (e.

.lead), givesrise to

secondaryemissionofX-rays viaaprocessknownasBremsstrahlung, meaning braking

radiation. Thereforeshielding must beaccomplished with low density

materials, e.

.Plexiglas, Lucite, plastic, wood, orwater.[20]

33

P, a beta-emitter (0.25 MeV) withahalf-lifeof25.4days. It isused in life-science laboratories in

applications in which lowerenergy betaemissionsareadvantageoussuchas DNA sequencing.

[edit] hemical propertiesSeealso: Category:Phosphoruscompounds

Hydrides:PH3,P2H4

Halides:PBr5, PBr3, P

l3, PI3

xides:P4O6, P4O10

Sulfides:P4S6, P4S10

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Acids:H3PO2, H3PO4

Phosphates:(NH4)3PO4, a3(PO4)2, ePO4, e3(PO4)2,Na3PO4, a(H2PO4)2, KH2PO4

Phosphides:

a3P2, GaP,

n3P2 u3P

Organophosphorusandorganophosphates:Lawesson's

reagent, Parathion, Sarin, Soman, Tabun, Triphenyl phosphine, VXnerve gas[edit]Chemical bonding

Formoredetailson this topic, seeOctetrule.

Becausephosphorus is just below nitrogen in theperiodic table, the twoelementssharemanyof their

bonding characteristics.

or instance, phosphine, PH3, isananalogueofammonia, NH3. Phosphorus,

likenitrogen, is trivalent in thismolecule.

The "trivalent" orsimple 3-bond view is thepre-quantummechanical Lewisstructure, whichalthough

somewhat ofasimplification fromaquantumchemical point of view, illustratessomeof the

distinguishing chemistryof theelement. Inquantumchemical valence bond theory, the valence

electronsareseen to be inmixturesof foursandpatomicorbitals, so-calledhybrids. In this view, the

threeunpairedelectrons in the three 3porbitalscombine with the twoelectrons in the 3sorbital to

form threeelectronpairsofoppositespin, available forthe formationof three bonds. Theremaining

hybridorbital contains twopairednon-bonding electrons, whichshow asa lonepairin the Lewis

structure.

Thephosphoruscation is verysimilarto thenitrogencation. In thesame way that nitrogen forms the

tetravalent ammonium ion, phosphoruscan form the tetravalent phosphonium ion, and formsalts

suchasphosphonium iodide[PH4]+[I

].

Likeotherelements in the thirdorlowerrowsof theperiodic table, phosphorusatomscanexpand

theirvalence tomakepenta- andhexavalent compounds. Thephosphoruschloridemolecule isan

example.

hen thephosphorus ligandsarenot identical, themoreelectronegative ligandsare

located in theapical positionsand the least electronegative ligandsare located in theaxial positions.

ithstronglyelectronegative ions, inparticularfluorine, hexavalencyas in P

6occursas well. This

octahedral ion isisoelectronic with S 6. In the bonding thesix octahedral sp

3d

2hybridatomicorbitals

playan important role.

Beforeextensivecomputercalculations were feasible, it was generallyassumed that the

nearbyd

orbitals in then

= 3 shell were theobviouscauseof thedifference in binding betweennitrogenandphosphorus (i.e., phosphorushad 3dorbitalsavailable for3sand 3pshell bonding

electronhybridisation, but nitrogendidnot). However, in theearlyeighties the German theoretical

chemist

ernerKutzelnigg[21]

found fromananalysisofcomputercalculations that thedifference in

binding ismore likelydue todifferences incharacterbetween the valence2pand valence 3porbitals

ofnitrogenandphosphorus, respectively. The2sand2porbitalsof first row atomsare localized in

roughly thesameregionofspace, while the 3porbitalsofphosphorusaremuchmoreextended in

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space. The violationof theoctet ruleobserved incompoundsofphosphorus is thendue to thesizeof

thephosphorusatom, and thecorresponding reductionofsterichindrance between its ligands. In

modern theoretical chemistry, Kutzelnigg'sanalysis is generallyaccepted.

ThesimpleLewisstructure forthetrigonal bipyramidalP l5moleculecontains fivecovalent bonds,

implying ahypervalent molecule with ten valenceelectronscontrary to theoctet rule.

Analternatedescriptionof the bonding, however, respects theoctet rule byusing 3-centre-4-electron

(3c-4e) bonds. In thismodel theoctet on the P atomcorresponds tosix electrons which form three

Lewis (2c-2e) bonds to the threeequatorial

l atoms, plus the twoelectrons in the 3-centre

l-P-

l

bonding molecularorbital forthe twoaxial

l electrons. The twoelectrons in thecorresponding

nonbonding molecularorbital arenot included because thisorbital is localizedon the two

l atoms

anddoesnot contribute to theelectrondensityon thephosphorusatom. (However, it shouldalways

beremembered that theoctet rule isnot someuniversal ruleofchemical bonding, and whilemany

compoundsobey it, therearemanyelements to which it doesnot apply).

[edit]Phosphine, diphosphine and phosphonium salts

Phosphine (PH3)andarsine (AsH3)arestructural analogues withammonia (NH3)and formpyramidal

structures with thephosphorusorarsenicatom in thecentre bound to threehydrogenatomsandone

loneelectronpair. Botharecolourless, ill-smelling, toxiccompounds. Phosphine isproduced ina

mannersimilarto theproductionofammonia. Hydrolysisofcalciumphosphide,

a3P2, orcalcium

nitride,

a3N2producesphosphineorammonia, respectively.

nlikeammonia, phosphine isunstable

and it reacts instantly withairgiving offphosphoricacidclouds. Arsine iseven lessstable. Although

phosphine is less basic thanammonia, it can formsomephosphoniumsalts (like PH4I), analoguesof

ammoniumsalts, but thesesalts immediatelydecompose in wateranddonot yieldphosphonium(PH4

+) ions. Diphosphine (P2H4orH2P-PH2) isananalogueofhydrazine (N2H4) that isacolourless

liquid whichspontaneously ignites inairandcandisproportionate intophosphineandcomplex

hydrides.

[edit]Halides

The trihalidesP 3, P l3, PBr3andPI3and thepentahalides, P l5andPBr5areall knownandmixed

halidescanalso be formed. The trihalidescan be formedsimply bymixing theappropriate

stoichiometricamountsofphosphorusandahalogen.orsafetyreasons, however, P

3 is typically

made byreacting P

l3 withAsF5and fractional distillation because thedirect reactionofphosphorus

with fluorinecan beexplosive. Thepentahalides, PX5, aresynthesized byreacting excesshalogen

witheitherelemental phosphorusorwith thecorresponding trihalide. Mixedphosphorushalidesare

unstableanddecompose to formsimplehalides. Thus 5PF3Br2decomposes into 3PF5and2PBr5.

[edit]Oxides and oxyacids

Phosphorus(III)oxide, P4O6 (alsocalled tetraphosphorushexoxide)andphosphorus(IV)oxide,

P4O10 (or tetraphosphorusdecoxide)areacidanhydridesofphosphorusoxyacidsandhencereadily

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withurine, whichcontainsconsiderablequantitiesofdissolvedphosphates fromnormal

metabolism.[4]

orking inHamburg, Brandattempted tocreate the fabledphilosopher'sstone through

thedistillationofsomesalts byevaporating urine, and in theprocessproduceda whitematerial that

glowed in thedarkand burned brilliantly. Hisprocessoriginally involved letting urinestand fordays

until it gaveoffa terriblesmell. Thenhe boiled it down toapaste, heated thispaste toahightemperature, and led the vapours through water, wherehehoped they wouldcondense to gold.

Instead, heobtaineda white, waxysubstance that glowed in thedark. Brandhaddiscovered

phosphorus, the first element discoveredsinceantiquity.

enow know that Brandproduced

ammoniumsodiumhydrogenphosphate, (NH4)NaHPO4. hile thequantities wereessentiallycorrect

(it tookabout 1,100 L ofurine tomakeabout 60 g ofphosphorus), it wasunnecessary toallow the

urine torot. Laterscientists woulddiscover that freshurineyielded thesameamount ofphosphorus.

Since that time, phosphorsandphosphorescencewereused loosely todescribesubstances that

shine in thedark without burning. However, asmentionedabove, even though the term

phosphorescence wasoriginallycoinedasa term byanalogy with the glow fromoxidationof

elemental phosphorus, isnow reserved foranotherfundamentallydifferent processre-emissionof

light after illumination.

Phosphorus was graduallyrecognizedasachemical element in itsownright at theemergenceof

theatomic theory that graduallyoccurred in the latepart of the 18thcenturyand theearly 19th

century (see

ohn Dalton formorehistory).

Brandat first tried tokeep themethodsecret,[23]

but latersold therecipe for200 thalerto D Krafft from

Dresden,[4]

whocouldnow make it as well, and touredmuchof Europe with it, including England,

wherehemet withRobert Boyle. Thesecret that it wasmade fromurine leakedout and firstohann

Kunckel (1630-1

03) in Sweden (16

8)and laterBoyle in London (1680)alsomanaged tomake

phosphorus. Boylestates that Krafft gavehimno informationas to thepreparationofphosphorus

other than that it wasderived from "somewhat that belonged to the bodyofman". This gave Boylea

valuableclue, however, so that he, too, managed tomakephosphorus, andpublished themethodof

itsmanufacture.[4]

Laterhe improved Brand'sprocess byusing sand in thereaction (still using urine

as basematerial),

4 NaPO3 + 2 SiO2 + 10

2 Na2SiO3 + 10

O + P4

Robert Boyle was the first tousephosphorus to ignitesulfur-tipped woodensplints, forerunners

ofourmodernmatches, in 1680.

In 1

69ohan Gottlieb Gahnand

arl

ilhelm Scheeleshowed that calciumphosphate

(

a3(PO4)2) is found in bones, and theyobtainedphosphorus from boneash.Antoine

Lavoisierrecognizedphosphorusasanelement in 1

. Boneash was themajorsourceof

phosphorusuntil the 1840s. Phosphaterock, amineral containing calciumphosphate, was first

used in 1850 and following the introductionof theelectricarc furnace in 1890, this became the

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onlysourceofphosphorus. Phosphorus, phosphatesandphosphoricacidarestill obtained from

phosphaterock. Phosphaterock isamajorfeedstock in the fertilizer industry.

Earlymatchesused whitephosphorus in theircomposition, which wasdangerousdue to its

toxicity. Murders, suicidesandaccidental poisoningsresulted from itsuse. (Anapocryphal tale

tellsofa womanattempting tomurderherhusband with whitephosphorus inhis food, which

wasdetected by thestew giving off luminoussteam).[7]

Inaddition, exposure to the vapours

gavematch workersaseverenecrosisof the bonesof the jaw, the infamous "phossy jaw".

henasafeprocess formanufacturing redphosphorus wasdiscovered, with its farlower

flammabilityand toxicity, laws wereenacted, under theBerne

onvention (1906), requiring its

adoptionasasaferalternative formatchmanufacture.[12]

[edit]Occurrence

Seealso: category:Phosphateminerals

Due to itsreactivity withairandmanyotheroxygen-containing substances, phosphorus isnot

found free innature but it is widelydistributed inmanydifferent minerals.

Phosphaterock, which ispartiallymadeofapatite (an impure tri-calciumphosphatemineral), is

an important commercial sourceof thiselement. About 50 percent of the global phosphorus

reservesare in the Arab nations.[24]

Largedepositsofapatiteare located

in

hina, Russia, Morocco, Florida, Idaho, Tennessee,

tah, andelsewhere.Albright and

ilson in the

nited Kingdomand theirNiagaraFallsplant, for instance, wereusing phosphate

rock in the 1890sand 1900s from

onnetable, TennesseeandFlorida; by 1950 they wereusing

phosphaterockmainly from Tennesseeand North Africa.[13]

In theearly 1990s Albright and

ilson'spurified wet phosphoricacid business was being adverselyaffected byphosphaterock

sales by

hinaand theentryof their long-standing Moroccanphosphatesuppliers into the

purified wet phosphoricacid business.[25]

In2007, at thecurrent rateofconsumption, thesupplyofphosphorus wasestimated torunout

in 345 years.[26]

However, scientistsarenow claiming that a "Peak Phosphorus" will occurin 30

yearsand that "At current rates, reserves will bedepleted in thenext 50 to 100 years."[27]

[edit]Production

hitephosphorus was first madecommercially, forthematch industry in the 19thcentury, by

distilling offphosphorus vapour fromprecipitatedphosphates, mixed with groundcoal

orcharcoal, which washeated inan ironpot, inretort.[28]

Theprecipitatedphosphates weremade

from ground-up bones that had beende-greasedand treated withstrong acids.

arbon

monoxideandotherflammable gasesproducedduring thereductionprocess were burnt off ina

flarestack.

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This process ecame o solete in the late 1890s hen theelectric arc furnace as adapted to

reduce phosphate rock.[29][30]

Calcium phosphate

phosphate rock), mostly mined in Florida and

orth Africa, can

e heated to 1,200-1,500 C

ith sand,

hich is mostly SiO2, and coke

impure

car

on) to produceapori

ed tetraphosphorus, P4,

mp. 44.2 C)

hich is su

sequently

condensed into a

hite po

der under

ater to pre

ent o

idation. E

en under

ater,

hitephosphorus is slo

ly con

erted to the more sta

le red phosphorusallotrope

mp. 597 C). Both

the

hite and red allotropes of phosphorus are insolu

le in

ater.

The electric furnace method allo ed production to increase to the point here phosphorus could

e used in

eapons of

ar.

[7][13]In World War I it

as used in incendiaries, smoke screensand

tracer ullets.[13]

A special incendiary ullet as de eloped to shoot athydro en-

filled ZeppelinsoerBritain

hydro

enein

hi

hly inflamma

le if it can

e

i

nited).[13]

urinWorld War II,

oloto

cocktails ofen

ene and phosphorus

ere distri

uted

in Britain to specially selected ciilians

ithin the British resistance operation, for defence; and

phosphorus incendiary om s ere used in ar on a lar e scale. Burnin phosphorus is difficult

to etin

uish and if it splashes onto human skin it has horrific effects

see precautions

elo

).[12]

Today phosphorus production is lar er than e er. It is used as a precursorfor arious

chemicals,[31]

in particular the her

icidelyphosate sold under the

rand name

oundup.

Production of

hite phosphorus takes place at lar

e facilities and it is transported heated in

liquid form. Some major accidents hae occurred durin

transportation, train derailments

at Bro

nston,

e

raska and

iamis

ur

, Ohio led to lar

e fires. The orst accident in recent

times

as an enironmental one in 1968

hen phosphorus spilled into the sea from a plant

at Placentia Bay, e foundland.[32]

[edit]Applications

atch strikin surface made of a mi

ture of red phosphorus, lue and round lass. The lass is used to

increase the friction.)

Widely used compounds Use

Ca(H2PO4)2H2O Baking powder & fertilizers

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CaHPO42H2O Animal food additive,toothpowder

H3PO4 Manufacture of phosphate fertili ers

PCl3 Manufacture ofPOCl3and pesticides

POCl3 Manufacturing plastici er

P4S10 Manufacturing ofadditives and pesticides

Na5P3O10 Detergents

Phosphorus, being anessential plant nutrient, finds itsmajoruseasaconstituent

offertilizers foragricultureand farmproduction in the formofconcentratedphosphoricacids,

whichcanconsist of70% to75% P2O5. Global demand forfertilizers led to large increase

inphosphate (PO43-)production in thesecondhalfof the20thcentury. Due to theessential

natureofphosphorus to living organisms, the low solubilityofnatural phosphorus-containing

compounds, and theslow natural cycleofphosphorus, theagricultural industry isheavilyreliant

on fertilizers whichcontainphosphate, mostly in the formofsuperphosphateof lime.

Superphosphateof lime isamixtureof twophosphatesalts, calciumdihydrogenphosphate

a(H2PO4)2andcalciumsulfatedihydrate

aSO42H2Oproduced by thereactionofsulfuricacid

and waterwithcalciumphosphate.

Phosphorus is widelyused tomakeorganophosphoruscompounds, through the

intermediatesphosphoruschloridesand twophosphorussulfides:phosphoruspentasulfide,

andphosphorussesquisulfide.[13]

Organophosphoruscompoundshavemanyapplications,

including inplasticizers, flameretardants, pesticides, extractionagents, andwater

treatment.[12]

Phosphorus isalsoan important component insteelproduction, in themaking ofphosphor

bronze, and inmanyotherrelatedproducts.

Phosphatesareutilized in themaking ofspecial glasses that areused forsodium lamps.[33]

Bone-ash, calciumphosphate, isused in theproductionof finechina.[33]

Sodium tripolyphosphatemade fromphosphoricacid isused in laundrydetergents insome

countries, but banned forthisuse inothers.[33]

Phosphoricacidmade fromelemental phosphorus isused in foodapplicationssuchassome

soda beverages. Theacid isalsoastarting point tomake food gradephosphates.[13]

These

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includemono-calciumphosphate which isemployed inbaking powderandsodium

tripolyphosphateandothersodiumphosphates[13]

. Among otheruses theseareused to

improve thecharacteristicsofprocessedmeat andcheese. Othersareused in

toothpaste.[13]

Trisodiumphosphate isused incleaning agents tosoften waterand for

preventing pipe/boiler tubecorrosion. hitephosphorus, called " P" (slang term " illie Peter") isused inmilitaryapplications

asincendiary bombs, forsmoke-screeningassmokepotsandsmoke bombs, and intracer

ammunition. It isalsoapart ofanobsolete M34 hite Phosphorus S hand grenade. This

multipurpose grenade wasmostlyused forsignalling, smokescreensand inflammation; it

couldalsocausesevere burnsandhadapsychological impact on theenemy.[34][35]

Redphosphorus isessential formanufacturing matchbookstrikers, flares,[13]

safetymatches,

pharmaceutical gradeandstreet methamphetamine, and isused incap guncaps.

Phosphorussesquisulfide isused inheadsofstrike-anywherematches.[13]

In traceamounts, phosphorus isusedasadopant forn-typesemiconductors.

32

P and33

P areusedasradioactive tracers in biochemical laboratories (seeIsotopes).

[edit]Biological role

Phosphorus isakeyelement inall known formsoflife. Inorganicphosphorus in the formof the

phosphate PO43-

playsamajorrole in biological moleculessuchas DNA and RNA where it

formspart of thestructural frameworkof thesemolecules. Living cellsalsousephosphate to

transport cellularenergy in the formofadenosine triphosphate (ATP). Nearlyeverycellular

process that usesenergyobtains it in the formof ATP. ATP isalso important

forphosphorylation, akeyregulatoryevent incells. Phospholipidsare themainstructural

componentsofall cellularmembranes. alciumphosphatesaltsassist instiffening bones.[12]

Everycell hasamembrane that separates it from itssurrounding environment. Biological

membranesaremade fromaphospholipidmatrix andproteins, typically in the formofa bilayer.

Phospholipidsarederived fromglycerol, such that twoof the glycerol hydroxyl (OH)protons

have beenreplaced with fattyacidsasanester, and the thirdhydroxyl protonhas beenreplaced

withphosphate bonded toanotheralcohol.[12]

Anaverageadult humancontainsabout 0.7kg ofphosphorus, about 85-90% of which ispresent

in bonesand teeth in the formofapatite, and theremainder insoft tissuesandextracellular

fluids (~1%). Thephosphoruscontent increases fromabout 0.5 weight% in infancy to 0.65-1.1

weight% inadults. Averagephosphorusconcentration in the blood isabout 0.4 g/L, about 70%

of that isorganicand 30% inorganicphosphates.[36]

A well-fedadult in the industrialized world

consumesandexcretesabout 1-3 g ofphosphorusperday, withconsumption in the formof

inorganicphosphateandphosphorus-containing biomoleculessuchasnucleicacidsand

phospholipids;andexcretionalmost exclusively in the formofurinephosphate ion. Onlyabout

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0.1% of

ody phosphate circulates in thelood,

ut this amount reflects the amount of

phosphate aaila

le to soft tissue cells.

[12]

In medicine, lo

phosphate syndromes are caused

y malnutrition,

y failure to a

sor

phosphate, and y meta olic syndromes hich dra phosphate from the lood such as re-

feedin

after malnutrition) or pass too much of it into the urine. All are characteri

ed

y hypophosphatemia see article for medical details),

hich is a condition of lo

le

els of

solule phosphate le

els in the

lood serum, and therefore inside cells. Symptoms of

hypophosphatemia include muscle and neurolo

ical dysfunction, and disruption of muscle and

lood cells due to lack of ATP. Too much phosphate can lead to diarrhoea and calcification

hardenin

) of or

ans and soft tissue, and can interfere ith the ody's a ility to use iron,

calcium, ma

nesium, and

inc.[37]

Phosphorus is an essential macromineral for plants, hich is studied e tensi ely

in edapholo

y in order to understand plant uptake from soil systems. In ecolo

ical terms,

phosphorus is often a limitin

factorin many enironments; i.e. the a

aila

ility of phosphorus

oerns the rate of

ro

th of many or

anisms. In ecosystems an ecess of phosphorus can

e

pro

lematic, especially in aquatic systems, seeeutrophication and al

allooms.

[edit]Precautions

Or

anic compounds of phosphorus form a ide class of materials, some of hichare e tremely

toic. Fluorophosphateesters are amon

the most potent neurotoinskno

n. A

ide ran

e of

or

anophosphorus compounds are used for their toicity to certain or

anisms

as pesticides her icides, insecticides, fun

icides, etc.) and eaponised as ner e a

ents.

ost

inor

anic phosphates are relatiely nonto

ic and essential nutrients. For en

ironmentally

aderse effects of phosphates seeeutrophicationand al

al

looms.[12]

The hite phosphorus allotrope should e kept under ater at all times as it presents a

si

nificant fire ha

ard due to its etreme reacti

ity

ith atmospheric o

y

en, and it should only

e manipulated ith forceps since contact ith skin can cause se ere urns. Chronic hite

phosphorus poisonin

leads to necrosis of the ja

called

phossy ja

. In

estion of

hite

phosphorus may cause a medical condition kno

n asSmokin

Stool Syndrome.[38]

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When the

hite form is e

posed to sunliht or

hen it is heated in its o

n

apour to 250C, it is

transmuted to the red form,

hich does not chemoluminesce in air. The red allotrope does not

spontaneously i

nite in air and is not as dan

erous as the

hite form.

e

ertheless, it should

e

handled

ith care

ecause it re

erts to

hite phosphorus in some temperature ran

es and it

also emits hi

hly to

ic fumes that consist of phosphorus o

ides

hen it is heated.

[12]

Phosphorus e

plosion

Upon e

posure to elemental phosphorus, in the past it as su ested to ash the affected area

ith 2% copper sulfate solution to form harmless compounds that can

e ashed a ay.

Accordin

to the recent USNavy's Treatment of

hemical Agent

asualties and

onventional

Military

hemical Injuries: FM8-285: Part2

onventionalMilitary

hemical Injuries,

Cupric

copper II)) sulfate has

een used

y U.S. personnel in the past and is still

ein used

y some

nations.

o

e

er, copper sulfate is to

ic and its use

ill

e discontinued. Copper sulfate may

produce kidney and cere

ral to

icity as

ell as intra

ascular hemolysis.[39]

The manual su ests instead

a

icar

onate solution to neutralie phosphoric acid,

hich

ill

then allo

remo

al of

isi

le

hite phosphorus. Particles often can

e located

y their emission

of smoke

hen air strikes them, or

y their phosphorescence in the dark. In dark surroundin

s,

fra

ments are seen as luminescent spots.

Then,

Promptly de

ride the

urn if the patient's

condition

ill permit remo

al of

its of WP

hich mi

ht

e a

sor

edlater and possi

ly produce

systemic poisonin

.

O

OT apply oily-based ointments until it is certain that all WP has been

remo

ed. Follo in complete remo

al of the particles, treat the lesions as thermal burns.[note

1]As

hite phosphorus readily mi

es

ith oils, any oily substances or ointments are not

recommended until the area is thorou hly cleaned and all hite phosphorus remo

ed.

[edit]US DEA ListIstatus

Phosphorus can reduce elemental iodine to hydroiodic acid,

hich is a rea

ent effecti

e forreducin

ephedrine orpseudoephedrine to methamphetamine.

[40]For this reason, t

o allotropes

of elemental phosphorus red phosphorus and hite phosphorus ere desi nated by the

United States

ru

Enforcement Administration as

ist I precursor chemicals under21 CF

1310.02 effectie on

o

ember17, 2001.

[41]As a result, in the United States, handlers of red

phosphorus or

hite phosphorus are subject to strin

ent re

ulatory controls pursuant to

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theControlled Substances Act in order to reduce di

ersion of these substances for use in

clandestine production of controlled substances.[41][42][43]

[edit]See also

White phosphorus

eapon)[edit] otes

1. ^This quote uses the ord

phosphorescence

,

hich is actually incorrect, WP,

White

Phosphorous), e hibits chemoluminescence upon e posure to air and if there is any

WP in the

ound, co

ered by tissue or fluids such as blood serum, it

ill not

chemoluminescence until it is mo

ed to a position

here the air can

et at it and

acti

ate the chemoluminescent

lo

hich requires a

ery dark room and dark adapted

eyes to see clearly.

Cate ory:Potassium compoundsFrom Wikipedia, the free encyclopedia

Wikimedia Commons has

media related to:Potassium

compounds

Potassium compoundsare those chemical compounds

hich contain the chemical

elementpotassium.

Subcate ories

This cate

ory has only the follo

in

subcate

ory.

P

[+] Potassium minerals 57 P, 1 F)

Pa es in cate ory Potassium compounds

The follo

in

92 pa

es are in this cate

ory, out of92 total. This list may not reflect recent chan

es

learn more).

A

Alkalide

P cont.

Potassium benzoate

P cont.

Potassium iodate

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C

Chrome alum

D

Dipotassium guanylate

Dipotassium phosphate

F

Fowler's solution

K

Krogmann's salt

L

Liver of sulfur

M

Monopotassium glutamate

Monopotassium phosphate

Monopotassium phosphite

N

Nessler's reagent

P

Potassium 2-ethylhexanoate

Potassium aluminate

Potassium ferrioxalate

Potassium ferrocyanide

Potassium fumarate

Potassium peroxide

Potassium

peroxymonosulfate

Potassium phosphate

Potassium sorbate

Potassium tartrate

Potassium acetate

Potassium adipate

Potassium alum

Potassium bicarbonate

Potassium bifluoride

Potassium bisulfate

Potassium bisulfite

Potassium bitartrate

Potassium bromate

Potassium bromide

Potassium canrenoate

Potassium carbonate

Potassium chlorate

Potassium chloride

Potassium chromate

Potassium citrate

Potassium cobaltinitrite

Template:Potassium compounds

Potassium cyanate

Potassium cyanide

Potassium dichromate

Potassium dideuterium

phosphate

Potassium ferrate

Potassium ferricyanide

Potassium fluoride

Potassium formate

Potassium fulminate

Potassium gluconate

Potassium hexachloroplatinate

Potassium hexafluorophosphate

Potassium hydride

Potassium hydrosulfide

Potassium hydroxide

Potassium iodide

Potassium malate

Potassium manganate

Potassium manganite

Potassium metabisulfite

Potassium nitrate

Potassium nitrite

Potassium octachlorodimolybdate

Potassium oxide

Potassium perchlorate

Potassium periodate

Potassium permanganate

Potassium persulfate

Potassium picrate

Potassium propionate

Potassium pyrosulfate

Potassium silicate

Potassium sodium tartrate

Potassium sulfate

Potassium sulfide

Potassium sulfite

Potassium superoxide

Potassium tetrachloroplatinate

Potassium

tetraperoxochromate(V)

Potassium tetraphenylborate

Potassium thiocyanate

Potassium titanyl phosphate

S

Salt substitute

T

Tripotassium phosphate

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Potassium aluminiumborate

Potassium aluminium

fluoride

Potassium amide

Potassium argentocyanide

Potassium arsenate

Potassium ascorbate

Potassium azide

Media incategory "Potassiumcompounds"

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