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==Overview==
'''Organophosphorus compounds''' are [[chemical compound]]s containing [[carbon]]-[[phosphorus]] [[chemical bond|bonds]]. '''Organophosphorus chemistry''' is the corresponding science exploring the properties and reactivity of organophosphorus compounds. Phosphorus shares [[nitrogen group|group 15]] in the periodic table with [[nitrogen]] and phosphorus compounds and nitrogen compounds have much in common.<ref>Dillon, K. B.; Mathey, F.; Nixon, J. F. ''Phosphorus. The Carbon Copy''; John Wiley & Sons, 1997. ISBN 0-471-97360-2</ref><ref>Quin, L. D. ''A Guide to Organophosphorus Chemistry''; John Wiley & Sons, 2000. ISBN 0-471-31824-8</ref>  
'''Organophosphorus compounds''' are [[chemical compound]]s containing [[carbon]]-[[phosphorus]] [[chemical bond|bonds]]. '''Organophosphorus chemistry''' is the corresponding science exploring the properties and reactivity of organophosphorus compounds. Phosphorus shares [[nitrogen group|group 15]] in the periodic table with [[nitrogen]] and phosphorus compounds and nitrogen compounds have much in common.<ref>Dillon, K. B.; Mathey, F.; Nixon, J. F. ''Phosphorus. The Carbon Copy''; John Wiley & Sons, 1997. ISBN 0-471-97360-2</ref><ref>Quin, L. D. ''A Guide to Organophosphorus Chemistry''; John Wiley & Sons, 2000. ISBN 0-471-31824-8</ref>  


Phosphorus can adopt [[oxidation state]]s &minus;3, &minus;1, 1, 3 and 5. In chemical literature very often compounds with +3 or &minus;3 oxidation state are grouped together as having a (III) oxidation state regardless of sign. In an official and more descriptive nomenclature phosphorus compounds are identified by their [[coordination number]] [[sigma|δ]] and their [[Valence (chemistry)|valency]] [[lambda|λ]]. In this system a phosphine is a δ<sup>3</sup>λ<sup>3</sup> compound.
Phosphorus can adopt [[oxidation state]]s &minus;3, &minus;1, 1, 3 and 5. In chemical literature very often compounds with +3 or &minus;3 oxidation state are grouped together as having a (III) oxidation state regardless of sign. In an official and more descriptive nomenclature phosphorus compounds are identified by their [[coordination number]] δ and their [[Valence (chemistry)|valency]] λ. In this system a phosphine is a δ<sup>3</sup>λ<sup>3</sup> compound.


== Phosphanes & phosphines ==
== Phosphanes & phosphines ==
The parent compound of the '''phosphanes''' is PH<sub>3</sub>, called phosphine in the US and UK and phosphane elsewhere.<ref> [[Gold Book]]: [http://www.iupac.org/goldbook/P04548.pdf Link]</ref>  Replacement of one or more protons by an organic residue, gives PH3-xR<sub>x</sub>, an organophosphine or organophosphane, again depending on the country.  The phosphorus atom in phosphanes/phosphines has a formal oxidation state &minus;3 (δ<sup>3</sup>λ<sup>3</sup>) and are the phosphorus analogues of simple [[amine]]s.
The parent compound of the '''phosphanes''' is PH<sub>3</sub>, called phosphine in the US and UK and phosphane elsewhere.<ref> [[Gold Book]]: [http://www.iupac.org/goldbook/P04548.pdf Link]</ref>  Replacement of one or more protons by an organic residue, gives PH3-xR<sub>x</sub>, an organophosphine or organophosphane, again depending on the country.  The phosphorus atom in phosphanes/phosphines has a formal oxidation state &minus;3 (δ<sup>3</sup>λ<sup>3</sup>) and are the phosphorus analogues of simple [[amine]]s.


An often used organic phosphine is [[triphenylphosphine]]. Like amines, phosphines have a [[trigonal pyramidal molecular geometry]] although with larger angles. The C-P-C [[bond angle]] is 98.6° for trimethylphosphine increasing to 109.7° when the methyl groups are replaced by [[tert-butyl|''tert''-butyl]] groups. Commonly the size of these ligands are described by the parameter called [[ligand cone angle|cone angle]].
An often used organic phosphine is [[triphenylphosphine]]. Like amines, phosphines have a trigonal pyramidal molecular geometry although with larger angles. The C-P-C [[bond angle]] is 98.6° for trimethylphosphine increasing to 109.7° when the methyl groups are replaced by [[tert-butyl|''tert''-butyl]] groups. Commonly the size of these ligands are described by the parameter called [[ligand cone angle|cone angle]].


The barrier to inversion is also much higher than in amines for a process like [[nitrogen inversion]] to occur and therefore phosphines with three different [[substituent]]s can display [[optical isomerism]].  
The barrier to inversion is also much higher than in amines for a process like [[nitrogen inversion]] to occur and therefore phosphines with three different [[substituent]]s can display [[optical isomerism]].  
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Amines and phosphines both have a [[lone pair]] of electrons but with a difference. Whereas the lone pair in an amine shares its electrons at every opportunity for [[delocalization]] for instance in [[pyridine]], the phosphorus atom in a similar configuration will not. For this reason, the phosphorus equivalent of [[pyrrole]] called [[phosphole]] is not at all [[aromatic]].     
Amines and phosphines both have a [[lone pair]] of electrons but with a difference. Whereas the lone pair in an amine shares its electrons at every opportunity for [[delocalization]] for instance in [[pyridine]], the phosphorus atom in a similar configuration will not. For this reason, the phosphorus equivalent of [[pyrrole]] called [[phosphole]] is not at all [[aromatic]].     


The reactivity of phosphines match that of amines with regard to [[nucleophilicity]] in the formation of [[Phosphonium salt]]s with the general structure PR<sub>4</sub><sup>+</sup>X<sup>&minus;</sup>. This property is used in the [[Appel reaction]] converting [[alcohol]]s to [[alkyl halide]]s.
The reactivity of phosphines match that of amines with regard to nucleophilicity in the formation of [[Phosphonium salt]]s with the general structure PR<sub>4</sub><sup>+</sup>X<sup>&minus;</sup>. This property is used in the [[Appel reaction]] converting [[alcohol]]s to [[alkyl halide]]s.
   
   
A difference in reactivity with amines is the ease of [[oxidation]] of phosphines to phosphine oxides.
A difference in reactivity with amines is the ease of [[oxidation]] of phosphines to phosphine oxides.
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* [[Nucleophilic displacement]] of phosphorous halides with organometallic reagents such as [[Grignard reagent]]s.
* [[Nucleophilic displacement]] of phosphorous halides with organometallic reagents such as [[Grignard reagent]]s.
* Nucleophilic displacement of metal phosphides, generated by reaction of potassium metal with phosphine as in [[sodium amide]] with [[alkyl halide]]s.
* Nucleophilic displacement of metal phosphides, generated by reaction of potassium metal with phosphine as in [[sodium amide]] with [[alkyl halide]]s.
*  [[Nucleophilic addition]] of phosphine with [[alkene]]s in presence of a strong base (often [[potassium hydroxide|KOH]] in [[dimethylsulfoxide|DMSO]]), [[Markovnikov's rule]]s apply.<ref>Arbuzova, S. N.; Gusarova, N. K.; Trofimov, B. A. "Nucleophilic and free-radical additions of phosphines and phosphine chalcogenides to alkenes and alkynes." ''[[Arkivoc]]'' '''2006''', part v, 12–36 (EL-1761AR). [http://www.arkat-usa.org/home.aspx?VIEW=MANUSCRIPT&MSID=1761 Article]</ref> Phosphine can be prepared in situ from [[red phosphorus]] and [[potassium hydroxide]]. Primary (RPH<sub>2</sub>) and secondary phospines (RRPH) do not require a base with electron-deficient alkenes such as [[acrylonitrile]]s.
*  [[Nucleophilic addition]] of phosphine with [[alkene]]s in presence of a strong base (often [[potassium hydroxide|KOH]] in [[dimethylsulfoxide|DMSO]]), [[Markovnikov's rule]]s apply.<ref>Arbuzova, S. N.; Gusarova, N. K.; Trofimov, B. A. "Nucleophilic and free-radical additions of phosphines and phosphine chalcogenides to alkenes and alkynes." ''Arkivoc'' '''2006''', part v, 12–36 (EL-1761AR). [http://www.arkat-usa.org/home.aspx?VIEW=MANUSCRIPT&MSID=1761 Article]</ref> Phosphine can be prepared in situ from red phosphorus and [[potassium hydroxide]]. Primary (RPH<sub>2</sub>) and secondary phospines (RRPH) do not require a base with electron-deficient alkenes such as [[acrylonitrile]]s.
 
[[Image:Phosphineadditionsalkenes.png|center|200px|Scheme 1. Addition of phosphine and phosphines to alkenes and alkynes]]


* [[Radical addition]] of phosphines to alkenes with [[AIBN]] or organic [[peroxide]]s to give anti-Markovnikov adducts.
* Radical addition of phosphines to alkenes with [[AIBN]] or organic [[peroxide]]s to give anti-Markovnikov adducts.
* [[Nucleophilic addition]] of phosphine and phosphines to [[alkyne]]s in presence of base. Secondary phosphines react with electron-deficient alkynes such as phenylcyanoacetylene without base.
* [[Nucleophilic addition]] of phosphine and phosphines to [[alkyne]]s in presence of base. Secondary phosphines react with electron-deficient alkynes such as phenylcyanoacetylene without base.
* [[Organic reduction]] of phosphine oxides for instance with [[chlorosilane]].  
* [[Organic reduction]] of phosphine oxides for instance with [[chlorosilane]].  
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* as nucleophiles for instance with [[alkyl halide]]s to [[phosphonium salt]]s. Phospines are key nucleophilic catalysts in the dimerization of enones in the [[Rauhut-Currier reaction]].
* as nucleophiles for instance with [[alkyl halide]]s to [[phosphonium salt]]s. Phospines are key nucleophilic catalysts in the dimerization of enones in the [[Rauhut-Currier reaction]].
* as reducing agents:  
* as reducing agents:  
:Phosphines are [[reducing agent]]s in the [[Staudinger reduction]] converting azides to amines and in the [[Mitsunobu reaction]] converting alcohols into esters. In these processes the phosphine is oxidized to the phosphine oxide. Phosphines have also been found to reduce activated carbonyl groups for instance the reduction of an α-keto ester to an α-hydroxy ester in ''scheme 2''.<ref>Zhang, W.; Shi, M. "Reduction of activated carbonyl groups by alkyl phosphines: formation of α-hydroxy esters and ketones." ''[[Chemical Communications|Chem. Commun.]]'' '''2006''', 1218–1220. {{DOI|10.1039/b516467b}}</ref> In the proposed [[reaction mechanism]] the first proton is on loan from the methyl group in trimethylphosphine (triphenylphosphine does not react).   
:Phosphines are [[reducing agent]]s in the [[Staudinger reduction]] converting azides to amines and in the [[Mitsunobu reaction]] converting alcohols into esters. In these processes the phosphine is oxidized to the phosphine oxide. Phosphines have also been found to reduce activated carbonyl groups for instance the reduction of an α-keto ester to an α-hydroxy ester in ''scheme 2''.<ref>Zhang, W.; Shi, M. "Reduction of activated carbonyl groups by alkyl phosphines: formation of α-hydroxy esters and ketones." ''Chem. Commun.'' '''2006''', 1218–1220. {{DOI|10.1039/b516467b}}</ref> In the proposed [[reaction mechanism]] the first proton is on loan from the methyl group in trimethylphosphine (triphenylphosphine does not react).   
:[[Image:Phosphine ester reduction.png|350px|center|Scheme 2. Reduction of activated carbonyl groups by alkyl phosphines]]


:When modified with suitable substituents as in certain ''diazaphospholenes'' (''scheme 3'') the polarity of the P-H bond can actually be inverted (see: [[umpolung]]) and the resulting phosphine [[hydride]] can reduce a carbonyl group as in the example of [[benzophenone]] in yet another way.<ref>Burck, S.; Gudat, D.; Nieger, M.; Du Mont, W.-W. "''P''-Hydrogen-Substituted 1,3,2-Diazaphospholenes: Molecular Hydrides." ''[[Journal of the American Chemical Society|J. Am. Chem. Soc.]]'' '''2006''', ''128'', 3946–3955. {{DOI|10.1021/ja057827j}}</ref>  
:When modified with suitable substituents as in certain ''diazaphospholenes'' (''scheme 3'') the polarity of the P-H bond can actually be inverted (see: [[umpolung]]) and the resulting phosphine [[hydride]] can reduce a carbonyl group as in the example of [[benzophenone]] in yet another way.<ref>Burck, S.; Gudat, D.; Nieger, M.; Du Mont, W.-W. "''P''-Hydrogen-Substituted 1,3,2-Diazaphospholenes: Molecular Hydrides." ''J. Am. Chem. Soc.'' '''2006''', ''128'', 3946–3955. {{DOI|10.1021/ja057827j}}</ref>  
    
    
[[Image:Phosphine umpolung.png|350px|center|Scheme 3. diazaphospholene phosphine hydride]]


* Multidentate phosphines such as [[BINAP]] are important [[ligand]]s in organometallic chemistry.
* Multidentate phosphines such as [[BINAP]] are important [[ligand]]s in organometallic chemistry.


===Phosphanes===
===Phosphanes===
Primary phosphanes are under-used in chemistry due to their general lack of stability towards oxygen. One study<ref>''Taming a Functional Group: Creating Air-Stable, Chiral Primary Phosphanes '' Rachel M. Hiney, Lee J. Higham, Helge Müller-Bunz, Declan G. Gilheany [[Angewandte Chemie International Edition]] Volume 45, Issue 43 , Pages 7248 - 7251 '''2006''' {{DOI|10.1002/anie.200602143}}</ref> reports on several novel air-stable aromatic primary phosphanes prepared by [[organic reduction]] of the corresponding  [[phosphonate]]:   
Primary phosphanes are under-used in chemistry due to their general lack of stability towards oxygen. One study<ref>''Taming a Functional Group: Creating Air-Stable, Chiral Primary Phosphanes '' Rachel M. Hiney, Lee J. Higham, Helge Müller-Bunz, Declan G. Gilheany Angewandte Chemie International Edition Volume 45, Issue 43 , Pages 7248 - 7251 '''2006''' {{DOI|10.1002/anie.200602143}}</ref> reports on several novel air-stable aromatic primary phosphanes prepared by [[organic reduction]] of the corresponding  [[phosphonate]]:   
 
[[Image:PhosphaneStability2.png|400px|center|Scheme 3b. Phosphane Stability]]


The stability is attributed to [[conjugated system|conjugation]] between the [[aromaticity|aromatic ring]] and the phosphorus [[lone pair]].
The stability is attributed to [[conjugated system|conjugation]] between the [[aromaticity|aromatic ring]] and the phosphorus [[lone pair]].
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'''Phosphine oxides''' (designation δ<sup>3</sup>λ<sup>3</sup>) have the general structure R<sub>3</sub>P=O with formal oxidation state &minus;1. Phosphines form [[hydrogen bond]]s and many phosphines are therefore soluble in water. The P=O bond is very polar with a [[dipole moment]] of 4.51 D for triphenylphosphine.  
'''Phosphine oxides''' (designation δ<sup>3</sup>λ<sup>3</sup>) have the general structure R<sub>3</sub>P=O with formal oxidation state &minus;1. Phosphines form [[hydrogen bond]]s and many phosphines are therefore soluble in water. The P=O bond is very polar with a [[dipole moment]] of 4.51 D for triphenylphosphine.  


The nature of the phosphorus to oxygen double bond is a matter of debate. Pentavalent phosphorus like nitrogen is not compatible with the [[octet rule]]. In older literature the bond is represented as a [[dative bond]] just like an [[amine oxide]]. The prevailing view is that of a full double bond with [[back bonding]] taking place between a filled oxygen electron pair and an empty phosphorus d-orbital (lacking in nitrogen). problem is: the P=O bond does not react as any C=C double bond as [[addition reaction]]s are absent and involvement of a phosphorus d-orbital in bonding is not supported [[in silico]]. Alternative theories favor an [[ionic bond]] P<sup>+</sup>&minus;O<sup>&minus;</sup> which on its own strength should explain the short [[bond length]]. [[Molecular Orbital Theory]] proposes that the short bond length is attributed to the donation of the lone pair electrons from oxygen to the antibonding phosphorus-carbon bonds. This proposal is supported by ''ab initio'' calculations and has gained consensus in the chemistry community.         
The nature of the phosphorus to oxygen double bond is a matter of debate. Pentavalent phosphorus like nitrogen is not compatible with the [[octet rule]]. In older literature the bond is represented as a dative bond just like an [[amine oxide]]. The prevailing view is that of a full double bond with back bonding taking place between a filled oxygen electron pair and an empty phosphorus d-orbital (lacking in nitrogen). problem is: the P=O bond does not react as any C=C double bond as [[addition reaction]]s are absent and involvement of a phosphorus d-orbital in bonding is not supported [[in silico]]. Alternative theories favor an [[ionic bond]] P<sup>+</sup>&minus;O<sup>&minus;</sup> which on its own strength should explain the short [[bond length]]. Molecular Orbital Theory proposes that the short bond length is attributed to the donation of the lone pair electrons from oxygen to the antibonding phosphorus-carbon bonds. This proposal is supported by ''ab initio'' calculations and has gained consensus in the chemistry community.         


Phosphines are easily oxidized to phosphine oxides as examplified by the directed synthesis of a phospha crown, the phosphorus analogue of an [[aza crown]]<ref>Edwards, P. G.; Haigh, R.; Li, D.; Newman, P. D. "Template Synthesis of 1,4,7-Triphosphacyclononanes." [[J. Am. Chem. Soc.]] '''2006''', ''128'', 3818–3830. {{DOI|10.1021/ja0578956}}</ref> where it is not possible to isolate the phosphine itself.<ref>In step 1 diphosphinoethane coordinates to a [[ferrocene]] containing additional [[carbon monoxide]] ligands and an [[acetonitrile]] ligand. The next step is a hydrophosphination with trivinylphosphine followed by [[alkylation]] with ethyl bromide and [[hydrogenation]] with hydrogen over [[palladium on carbon]]. In the final step the iron template is removed by [[bromine]] but oxidation of the phosphine groups is unavoidable</ref>  
Phosphines are easily oxidized to phosphine oxides as examplified by the directed synthesis of a phospha crown, the phosphorus analogue of an aza crown<ref>Edwards, P. G.; Haigh, R.; Li, D.; Newman, P. D. "Template Synthesis of 1,4,7-Triphosphacyclononanes." J. Am. Chem. Soc. '''2006''', ''128'', 3818–3830. {{DOI|10.1021/ja0578956}}</ref> where it is not possible to isolate the phosphine itself.<ref>In step 1 diphosphinoethane coordinates to a [[ferrocene]] containing additional [[carbon monoxide]] ligands and an [[acetonitrile]] ligand. The next step is a hydrophosphination with trivinylphosphine followed by [[alkylation]] with ethyl bromide and [[hydrogenation]] with hydrogen over [[palladium on carbon]]. In the final step the iron template is removed by [[bromine]] but oxidation of the phosphine groups is unavoidable</ref>  
 
[[Image:Phosphacrown.png|center|500px|Scheme 4. Phosphacrown]]


== Phosphonates ==
== Phosphonates ==
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== Phosphite and phosphate esters ==
== Phosphite and phosphate esters ==
[[Phosphite ester]]s or phosphites have the general structure P(OR)<sub>3</sub> with oxidation state +3. Phosphites are employed in the [[Perkow reaction]] and the [[Arbusov reaction]]. [[Organophosphate|Phosphate ester]]s with the general structure P(=O)(OR)<sub>3</sub> and oxidation state +5 are of great technological importance as [[flame retardant]] agents and [[plasticizer]]s. Lacking a P&minus;C bond, these compounds are technically not organophosphorus compounds.
[[Phosphite ester]]s or phosphites have the general structure P(OR)<sub>3</sub> with oxidation state +3. Phosphites are employed in the [[Perkow reaction]] and the Arbusov reaction. [[Organophosphate|Phosphate ester]]s with the general structure P(=O)(OR)<sub>3</sub> and oxidation state +5 are of great technological importance as [[flame retardant]] agents and [[plasticizer]]s. Lacking a P&minus;C bond, these compounds are technically not organophosphorus compounds.


== Phosphoranes ==
== Phosphoranes ==
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The first phosphaalkene was synthesised in 1974 by Becker as a [[keto-enol tautomerism]] akin a [[Brook rearrangement]]:
The first phosphaalkene was synthesised in 1974 by Becker as a [[keto-enol tautomerism]] akin a [[Brook rearrangement]]:
:[[Image:BeckerReaction.png|400px|Becker reaction to phosphaalkenes]]


with R = [[methyl]] or [[phenyl]] and tms representing [[trimethylsilyl]].
with R = [[methyl]] or [[phenyl]] and tms representing [[trimethylsilyl]].


In the same year [[Harold Kroto]] established spectroscopically that [[thermolysis]] of Me<sub>2</sub>PH yielded CH<sub>2</sub>=PMe.
In the same year [[Harold Kroto]] established spectroscopically that thermolysis of Me<sub>2</sub>PH yielded CH<sub>2</sub>=PMe.


A general method for the synthesis of phosphaalkenes is by [[elimination reaction|1,2-elimination]] of suitable precursors, initiated thermally or by base such as [[DBU (chemistry)|DBU]], [[DABCO]] or [[triethylamine]]:
A general method for the synthesis of phosphaalkenes is by [[elimination reaction|1,2-elimination]] of suitable precursors, initiated thermally or by base such as [[DBU (chemistry)|DBU]], [[DABCO]] or [[triethylamine]]:


:[[Image:PhosphaalkeneGeneral.png|400px|Phosphaalkene general method]]
The Becker method is used in the synthesis of the phosphorus pendant of [[Poly(p-phenylene vinylene)]]:<ref>''Phosphorus Copies of PPV: -Conjugated Polymers and Molecules Composed of Alternating Phenylene and Phosphaalkene Moieties'' Vincent A. Wright, Brian O. Patrick, Celine Schneider, and Derek P. Gates J. Am. Chem. Soc.; '''2006'''; 128(27) pp 8836 - 8844; (Article) {{DOI|10.1021/ja060816l}}</ref>
 
The Becker method is used in the synthesis of the phosphorus pendant of [[Poly(p-phenylene vinylene)]]:<ref>''Phosphorus Copies of PPV: -Conjugated Polymers and Molecules Composed of Alternating Phenylene and Phosphaalkene Moieties'' Vincent A. Wright, Brian O. Patrick, Celine Schneider, and Derek P. Gates [[J. Am. Chem. Soc.]]; '''2006'''; 128(27) pp 8836 - 8844; (Article) {{DOI|10.1021/ja060816l}}</ref>
 
:[[Image:Poly(p-phenylenephosphaalkene).png|400px|Poly(p-phenylenephosphaalkene)]]


[[Diphosphene]]s are compounds containing P=P phosphorus double bonds. [[Phosphazene]]s have a P=N double bond.
[[Diphosphene]]s are compounds containing P=P phosphorus double bonds. [[Phosphazene]]s have a P=N double bond.
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Overview

Organophosphorus compounds are chemical compounds containing carbon-phosphorus bonds. Organophosphorus chemistry is the corresponding science exploring the properties and reactivity of organophosphorus compounds. Phosphorus shares group 15 in the periodic table with nitrogen and phosphorus compounds and nitrogen compounds have much in common.[1][2]

Phosphorus can adopt oxidation states −3, −1, 1, 3 and 5. In chemical literature very often compounds with +3 or −3 oxidation state are grouped together as having a (III) oxidation state regardless of sign. In an official and more descriptive nomenclature phosphorus compounds are identified by their coordination number δ and their valency λ. In this system a phosphine is a δ3λ3 compound.

Phosphanes & phosphines

The parent compound of the phosphanes is PH3, called phosphine in the US and UK and phosphane elsewhere.[3] Replacement of one or more protons by an organic residue, gives PH3-xRx, an organophosphine or organophosphane, again depending on the country. The phosphorus atom in phosphanes/phosphines has a formal oxidation state −3 (δ3λ3) and are the phosphorus analogues of simple amines.

An often used organic phosphine is triphenylphosphine. Like amines, phosphines have a trigonal pyramidal molecular geometry although with larger angles. The C-P-C bond angle is 98.6° for trimethylphosphine increasing to 109.7° when the methyl groups are replaced by tert-butyl groups. Commonly the size of these ligands are described by the parameter called cone angle.

The barrier to inversion is also much higher than in amines for a process like nitrogen inversion to occur and therefore phosphines with three different substituents can display optical isomerism.

The basicity of phospines is less than that of corresponding amines, for instance phosphonium ion itself has a pKa of -14 compared to 9.21 for ammonium ion; trimethylphosphonium has a pKa of 8.65 compared to that of 9.76 of trimethylamine; and triphenylphosphonium (pKa 11.2) is less basic than triphenylammonium (pKa 19).

Amines and phosphines both have a lone pair of electrons but with a difference. Whereas the lone pair in an amine shares its electrons at every opportunity for delocalization for instance in pyridine, the phosphorus atom in a similar configuration will not. For this reason, the phosphorus equivalent of pyrrole called phosphole is not at all aromatic.

The reactivity of phosphines match that of amines with regard to nucleophilicity in the formation of Phosphonium salts with the general structure PR4+X−. This property is used in the Appel reaction converting alcohols to alkyl halides.

A difference in reactivity with amines is the ease of oxidation of phosphines to phosphine oxides.

Synthesis

Synthetic produces for phosphines are:

  • Radical addition of phosphines to alkenes with AIBN or organic peroxides to give anti-Markovnikov adducts.
  • Nucleophilic addition of phosphine and phosphines to alkynes in presence of base. Secondary phosphines react with electron-deficient alkynes such as phenylcyanoacetylene without base.
  • Organic reduction of phosphine oxides for instance with chlorosilane.

Reactions

The main reaction types of phosphines are:

Phosphines are reducing agents in the Staudinger reduction converting azides to amines and in the Mitsunobu reaction converting alcohols into esters. In these processes the phosphine is oxidized to the phosphine oxide. Phosphines have also been found to reduce activated carbonyl groups for instance the reduction of an α-keto ester to an α-hydroxy ester in scheme 2.[5] In the proposed reaction mechanism the first proton is on loan from the methyl group in trimethylphosphine (triphenylphosphine does not react).
When modified with suitable substituents as in certain diazaphospholenes (scheme 3) the polarity of the P-H bond can actually be inverted (see: umpolung) and the resulting phosphine hydride can reduce a carbonyl group as in the example of benzophenone in yet another way.[6]


  • Multidentate phosphines such as BINAP are important ligands in organometallic chemistry.

Phosphanes

Primary phosphanes are under-used in chemistry due to their general lack of stability towards oxygen. One study[7] reports on several novel air-stable aromatic primary phosphanes prepared by organic reduction of the corresponding phosphonate:

The stability is attributed to conjugation between the aromatic ring and the phosphorus lone pair.

Phosphine oxides

Phosphine oxides (designation δ3λ3) have the general structure R3P=O with formal oxidation state −1. Phosphines form hydrogen bonds and many phosphines are therefore soluble in water. The P=O bond is very polar with a dipole moment of 4.51 D for triphenylphosphine.

The nature of the phosphorus to oxygen double bond is a matter of debate. Pentavalent phosphorus like nitrogen is not compatible with the octet rule. In older literature the bond is represented as a dative bond just like an amine oxide. The prevailing view is that of a full double bond with back bonding taking place between a filled oxygen electron pair and an empty phosphorus d-orbital (lacking in nitrogen). problem is: the P=O bond does not react as any C=C double bond as addition reactions are absent and involvement of a phosphorus d-orbital in bonding is not supported in silico. Alternative theories favor an ionic bond P+−O− which on its own strength should explain the short bond length. Molecular Orbital Theory proposes that the short bond length is attributed to the donation of the lone pair electrons from oxygen to the antibonding phosphorus-carbon bonds. This proposal is supported by ab initio calculations and has gained consensus in the chemistry community.

Phosphines are easily oxidized to phosphine oxides as examplified by the directed synthesis of a phospha crown, the phosphorus analogue of an aza crown[8] where it is not possible to isolate the phosphine itself.[9]

Phosphonates

Phosphonates have the general structure R−P(=O)(OR)2. In the Horner-Wadsworth-Emmons reaction and the Seyferth-Gilbert homologation phosphonates are used as stabilized carbanions in reactions with carbonyl compounds. Phosphonates have many technical applications and bisphosphonates are a class of drugs.

Phosphite and phosphate esters

Phosphite esters or phosphites have the general structure P(OR)3 with oxidation state +3. Phosphites are employed in the Perkow reaction and the Arbusov reaction. Phosphate esters with the general structure P(=O)(OR)3 and oxidation state +5 are of great technological importance as flame retardant agents and plasticizers. Lacking a P−C bond, these compounds are technically not organophosphorus compounds.

Phosphoranes

Phosphoranes have a −5 oxidation state (δ5λ5) with parent compound the non-stable phosphoran PH5 or λ5-phosphane (lambda 5 phosphane). Phosphorus ylides are unsaturated phosphoranes used in the Wittig reaction.

Phosphorus multiple bonds

Many compounds exist with carbon phosphorus multiple bonds (P=C) as phosphaalkenes (R2C::PR) and phosphaalkynes (RC:::PR). In the compound phosphorine one carbon atom in benzene is replaced by phosphorus. The reactivity of phosphaalkenes is often compared to that of alkenes and not to that of imines. The reason is that the HOMO of phosphaalkenes is not the phosphorus lone pair (as in imines the amine lone pair) but the double bond. Therefore like alkenes, phosphaalkenes engage in Wittig reactions, Peterson reactions, Cope rearrangements and Diels-Alder reactions.

The first phosphaalkene was synthesised in 1974 by Becker as a keto-enol tautomerism akin a Brook rearrangement:

with R = methyl or phenyl and tms representing trimethylsilyl.

In the same year Harold Kroto established spectroscopically that thermolysis of Me2PH yielded CH2=PMe.

A general method for the synthesis of phosphaalkenes is by 1,2-elimination of suitable precursors, initiated thermally or by base such as DBU, DABCO or triethylamine:

The Becker method is used in the synthesis of the phosphorus pendant of Poly(p-phenylene vinylene):[10]

Diphosphenes are compounds containing P=P phosphorus double bonds. Phosphazenes have a P=N double bond.

See also

Template:ChemicalBondsToCarbon

External links

References

  1. ↑ Dillon, K. B.; Mathey, F.; Nixon, J. F. Phosphorus. The Carbon Copy; John Wiley & Sons, 1997. ISBN 0-471-97360-2
  2. ↑ Quin, L. D. A Guide to Organophosphorus Chemistry; John Wiley & Sons, 2000. ISBN 0-471-31824-8
  3. ↑ Gold Book: Link
  4. ↑ Arbuzova, S. N.; Gusarova, N. K.; Trofimov, B. A. "Nucleophilic and free-radical additions of phosphines and phosphine chalcogenides to alkenes and alkynes." Arkivoc 2006, part v, 12–36 (EL-1761AR). Article
  5. ↑ Zhang, W.; Shi, M. "Reduction of activated carbonyl groups by alkyl phosphines: formation of α-hydroxy esters and ketones." Chem. Commun. 2006, 1218–1220. doi:10.1039/b516467b
  6. ↑ Burck, S.; Gudat, D.; Nieger, M.; Du Mont, W.-W. "P-Hydrogen-Substituted 1,3,2-Diazaphospholenes: Molecular Hydrides." J. Am. Chem. Soc. 2006, 128, 3946–3955. doi:10.1021/ja057827j
  7. ↑ Taming a Functional Group: Creating Air-Stable, Chiral Primary Phosphanes Rachel M. Hiney, Lee J. Higham, Helge Müller-Bunz, Declan G. Gilheany Angewandte Chemie International Edition Volume 45, Issue 43 , Pages 7248 - 7251 2006 doi:10.1002/anie.200602143
  8. ↑ Edwards, P. G.; Haigh, R.; Li, D.; Newman, P. D. "Template Synthesis of 1,4,7-Triphosphacyclononanes." J. Am. Chem. Soc. 2006, 128, 3818–3830. doi:10.1021/ja0578956
  9. ↑ In step 1 diphosphinoethane coordinates to a ferrocene containing additional carbon monoxide ligands and an acetonitrile ligand. The next step is a hydrophosphination with trivinylphosphine followed by alkylation with ethyl bromide and hydrogenation with hydrogen over palladium on carbon. In the final step the iron template is removed by bromine but oxidation of the phosphine groups is unavoidable
  10. ↑ Phosphorus Copies of PPV: -Conjugated Polymers and Molecules Composed of Alternating Phenylene and Phosphaalkene Moieties Vincent A. Wright, Brian O. Patrick, Celine Schneider, and Derek P. Gates J. Am. Chem. Soc.; 2006; 128(27) pp 8836 - 8844; (Article) doi:10.1021/ja060816l

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