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Carbenium ion

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Methyl cation

A carbenium ion is a positive ion with the structure RR′R″C+, that is, a chemical species with one trivalent carbon that bears a +1 electric charge.

In older literature the name carbonium ion was used for this class, but now it refers exclusively to another family of carbocations, the carbonium ions, where the charged carbon is pentavalent.[1] The current definitions were proposed by the chemist George Andrew Olah in 1972,[2] and are now widely accepted.

Carbenium ions are generally highly reactive due to having an incomplete octet of electrons; however, certain carbenium ions, such as the tropylium ion, are relatively stable due to the positive charge being delocalised between the carbon atoms.

Nomenclature

Carbenium ions are classified as primary, secondary, or tertiary depending on whether the number of carbon atoms bonded to the ionized carbon is 1, 2, or 3. (Ions with zero carbons attached to the ionized carbon, such as methenium, CH+
3, are usually included in the primary class).

Reactivity

Stability typically increases with the number of alkyl groups bonded to the charge-bearing carbon. Tertiary carbocations are more stable (and form more readily) than secondary carbocations, because they are stabilized by hyperconjugation. Primary carbocations are highly unstable. Therefore, reactions such as the SN1 reaction and the E1 elimination reaction normally do not occur if a primary carbenium would be formed.

However, a carbon doubly bonded with the ionized carbon can stabilize the ion by resonance. Such cations as the allyl cation, CH
2=CH–CH+
2, and the benzyl cation, C
6H
5–CH+
2, are more stable than most other carbocations. Molecules which can form allyl or benzyl carbeniums are especially reactive. Carbenium ions can also be stabilized by heteroatoms.[3]

Carbenium ions may undergo rearrangement reactions from less stable structures to equally stable or more stable ones with rate constants in excess of 109 s−1. This fact complicates synthetic pathways to many compounds. For example, when 3-pentanol is heated with aqueous HCl, the initially formed 3-pentyl carbocation rearranges to a statistical mixture of the 3-pentyl and 2-pentyl. These cations react with chloride ion to produce about 1⁄3 3-chloropentane and 2⁄3 2-chloropentane.

Types of carbenium ions

Alkylium ions

Carbenium ions can be prepared directly from alkanes by removing a hydride anion, H−
, with a strong acid. For example, magic acid, a mixture of antimony pentafluoride (SbF
5) and fluorosulfuric acid (FSO
3H), turns isobutane into the cation (CH
3)
3C+
.[4]

Aromatic carbenium ions

Main article: Tropylium cation
Ball-and-stick model of the tropylium cation.

The tropylium ion is an aromatic species with the formula C
7H+
7.[5] Its name derives from the molecule tropine (itself named for the molecule atropine). Salts of the tropylium cation can be stable, e.g. tropylium tetrafluoroborate. It can be made from cycloheptatriene (tropylidene) and bromine or phosphorus pentachloride[6]

It is a heptagonal, planar, cyclic ion; it also has 6 π-electrons (4n + 2, where n = 1), which fulfills Hückel's rule of aromaticity. It can coordinate as a ligand to metal atoms.

The structure shown is a composite of seven resonance contributors in which each carbon carries part of the positive charge.

In 1891 G. Merling obtained a water-soluble salt from a reaction of cycloheptatriene and bromine.[7] The structure was elucidated by Eggers Doering and Knox in 1954.[8][9]

Another aromatic carbenium ion is the cyclopropenyl or cyclopropenium ion, C
3H+
3, obtained by Ronald Breslow and John T. Groves in 1970.[10] Though less stable than the tropylium cation, this carbenium ion can also from salts at room temperature. Solutions of such salts were found by Breslow and Groves to have spectroscopic and chemical properties matching expectations for an aromatic carbenium ion.

Triphenylmethyl (trityl) cation

Structure of triphenylmethyl hexafluorophosphate.

The triphenylmethyl cation, C(C6H5)3+, is especially stable because the positive charge can be distributed among 10 of the carbon atoms (the 3 carbon atoms in the ortho and para positions of each of the three phenyl groups, plus the central carbon atom). It exists in the compounds triphenylmethyl hexafluorophosphate (C(C6H5)3PF6) and triphenylmethyl perchlorate (C(C6H5)3ClO4).

Triphenylmethyl hexafluorophosphate is used as a catalyst and reagent in organic syntheses;[11] it is generated by combining silver hexafluorophosphate with triphenylmethyl chloride:[12]

AgPF6 + C(C6H5)3Cl → C(C6H5)3PF6 + AgCl

These and other similar cations can be obtained as intensely colored solutions by dissolving aryl-substituted methanols in concentrated sulfuric acid.[13]

Arenium ions

Main article: Arenium ion
Ball-and-stick model of the benzenium ion

An arenium ion is a cyclohexadienyl cation that appears as a reactive intermediate in electrophilic aromatic substitution.[14] For historic reasons this complex is also called a Wheland intermediate,[15] or a σ-complex.

benzenium ion

Two hydrogen atoms bonded to one carbon lie in a plane perpendicular to the benzene ring.[16] The arenium ion is no longer an aromatic species; however it is relatively stable due to delocalization: the positive charge is delocalized over 5 carbon atoms via the π system, as depicted on the following resonance structures:

Arenium ion resonance structures

Another contribution to the stability of arenium ions is the energy gain resulting from the strong bond between the benzene and the complexed electrophile.

The smallest arenium ion is protonated benzene, C
6H+
7. The benzenium ion can be isolated as a stable compound when benzene is protonated by the carborane superacid, H(CB11H(CH3)5Br6).[17] The benzenium salt is crystalline with thermal stability up to 150 °C. Bond lengths deduced from X-ray crystallography are consistent with a cyclohexadienyl cation structure.

Acylium ions

Main article: Acyl § Acylium cations, anions, and radicals

An acylium ion is a cation with the formula RCO+.[18] The structure is described as R−C≡O+ or R−C+=O. It is the synthetic and reactive equivalent of an acyl carbocation, but the actual structure has the oxygen and carbon linked by a triple bond. Such species are common reactive intermediates, for example, in the Friedel−Crafts acylations also in many other organic reactions such as the Hayashi rearrangement. Salts containing acylium ions can be generated by removal of the halide from acyl halides:

RC(O)Cl + SbCl5 → RCO+SbCl−
6

The C–O distance in these cations is near 1.1 ångströms, even shorter than that in carbon monoxide.[19] Acylium cations are characteristic fragments observed in EI-mass spectra of ketones.

See also

References

  1. ^ IUPAC Gold Book carbonium ion
  2. ^ "Stable carbocations. CXVIII. General concept and structure of carbocations based on differentiation of trivalent (classical) carbenium ions from three-center bound penta- of tetracoordinated (nonclassical) carbonium ions. Role of carbocations in electrophilic reactions" George Andrew Olah; J. Am. Chem. Soc.; 1972; 94(3); 808–820.
  3. ^ Hansjörg Grützmacher, Christina M. Marchand (1997), "Heteroatom stabilized carbenium ions", Coord. Chem. Rev., 163, 287–344. doi:10.1016/S0010-8545(97)00043-X
  4. ^ George A. Olah and Joachim Lukas (1967), "Stable Carbonium Ions. XLVII. Alkylcarbonium ion formation from alkanes via hydride (alkide) ion abstraction in fluorosulfonic acid-antimony pentafluoride-sulfuryl chlorofluoride solution". J. Am. Chem. Soc. 89 (18), 4739–4744. doi:10.1021/ja00994a030
  5. ^ IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version: (2006–) "molecule". doi:10.1351/goldbook.M04002
  6. ^ "Tropylium tetrafluorate" Organic Syntheses, Coll. Vol. 5, p.1138 (1973); Vol. 43, p.101 (1963). link
  7. ^ Merling, G. (1891), "Ueber Tropin". Berichte der deutschen chemischen Gesellschaft, 24: 3108–3126. doi:10.1002/cber.189102402151
  8. ^ "The Cycloheptatrienylium (Tropylium) Ion" W. von E. Doering, L. H. Knox J. Am. Chem. Soc., 1954, 76 (12), pp 3203–3206 doi:10.1021/ja01641a027
  9. ^ "Aromaticity as a Cornerstone of Heterocyclic Chemistry" Alexandru T. Balaban, Daniela C. Oniciu, Alan R. Katritzky Chem. Rev., 2004, 104 (5), 2777–2812 doi:10.1021/cr0306790
  10. ^ "Cyclopropenyl Cation. Synthesis and Characterization." R. Breslow and J. T. Groves J. Am. Chem. Soc. , 1970, 92 (4), 984–987 [1]
  11. ^ Urch, C. (2001). "Triphenylmethyl Hexafluorophosphate". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rt363f.
  12. ^ Sharp, D., Shepard, N. (1956). "Complex Fluorides. Part VIII". University Chemical Laboratory, Cambridge: 674–682.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  13. ^ N. C. Deno, J. J. Jaruzelski, and Alan Schriesheim (1955) "Carbonium ions. I. An acidity function (C0) derived from arylcarbonium ion equilibria." J. Am. Chem. Soc., 77 (11), 3044–3051. doi:10.1021/ja01616a036
  14. ^ "Stable carbocations. CXVIII. General concept and structure of carbocations based on differentiation of trivalent (classical) carbenium ions from three-center bound penta- of tetracoordinated (nonclassical) carbonium ions. Role of carbocations in electrophilic reactions" George A. Olah J. Am. Chem. Soc.; 1972; 94(3) 808–820; doi:10.1021/ja00758a020
  15. ^ "A Quantum Mechanical Investigation of the Orientation of Substituents in Aromatic Molecules" G. W. Wheland J. Am. Chem. Soc.; 1942; 64(4) 900–908; doi:10.1021/ja01256a047
  16. ^ A guidebook to mechanism in organic chemistry, Peter Sykes; pp 130–133
  17. ^ "Isolating Benzenium Ion Salts" Christopher A. Reed, Kee-Chan Kim, Evgenii S. Stoyanov, Daniel Stasko, Fook S. Tham, Leonard J. Mueller, and Peter D. W. Boyd J. Am. Chem. Soc.; 2003; 125(7) 1796–1804; doi:10.1021/ja027336o
  18. ^ Compendium of Chemical Terminology, acyl groups
  19. ^ B. Chevrier, J. M. Le Carpentier, R. Weiss "Synthesis of two crystalline species of the Friedel-Crafts intermediate antimony pentachloride-p-toluoyl chloride. Crystal structures of the donor-acceptor complex and of the ionic salt" J. Am. Chem. Soc., 1972, 94, 5718–5723.doi:10.1021/ja00771a031
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