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Non-coordinating ion

Introduction


Anions that interact weakly with cations are optimistically termed non-coordinating anions, although a more accurate term is ‘weakly coordinating anion’.[1] Non-coordinating anions are useful in studying the reactivity of electrophilic cations. They are commonly found as counterions for cationic metal complexes with an unsaturated coordination sphere. These special anions are essential components of homogeneous olefin polymerisation catalysts, where the active catalyst is a coordinatively unsaturated, cationic transition metal complex. For example, they are employed as counterions for the 14 valence electron cations [(C5H5)2ZrR]+ (R = methyl or a growing polyethylene chain).

Pre-“BARF” era

Pre-“BARF” era

Prior to the 1990s, BF4−, PF6−, and ClO4− were considered weakly-coordinating anions. These species are now known to bind well to electrophilic metal centers.[2] A particular problem inhibits the use of ClO4−, as its salts with organic cations are sometimes explosive. For this reason, perchlorate has almost fallen out of use due to safety concerns. Tetrafluoroborate and hexafluorophosphate anions are coordinating toward highly electrophilic metal ions, such as cations containing Zr(IV) centers, which can abstract fluoride from these anions. Other anions wee considered as low-coordinating with many cations, e.g., triflates for high-temperature applications.

Era of BARF

Era of BARF

A revolution in this area occurred in the 1990s with the introduction of [B[3,5-(CF3)2C6H3]4]−, commonly abbreviated as [BArF4]− and affectionately called “BARF.”[3]. This anion is far less coordinating than the tetrafluoroborate BF4−, hexafluorophosphate PF6−, and perchlorate ClO4−, consequently it has enabled the study of still more electrophilic cations.

File:NoncoordAnNew.png

In the tetraarylborates, the negative charge is symmetrically distributed over many electronegative atoms. Related anions are derived from tris(pentafluorophenyl)boron. Another advantage of these anions is that their salts are more soluble in non-polar organic solvents such as dichloromethane and, in some cases, even alkanes. Polar solvents, such as acetonitrile, THF, and water tend to bind to electrophilic centers, in which cases, the use of a noncoordinating anion is pointless.

Two publications describe pioneering results on “BARF”

  • The first preparation of B[3,5-(CF3)2C6H3]4−:

Nishida, H.; Takada, N.; Yoshimura, M.; Sonods, T.; Kobayashi, H. Bulletin of the Chemical Society of Japan 1984, volume 57, pp. 2600.

  • The preparation of [H(OCH2CH3)2]2]+B[3,5-(CF3)2C6H3]4−:Brookhart, M.; Grant, B.; Volpe, Jr., A. F.; Organometallics. 1992, volume 11, pp. 3920-3922.doi:10.1021/om00059a071.
Uses of non-coordinating anions

Uses of non-coordinating anions

Complexes derived from noncoordinating anions have been used to catalyze hydrogenation, hydrosilylation, oligomerization, and the living polymerization of olefins. The popularization of non-coordinating anions has contributed to increased understanding of agostic complexes wherein hydrocarbons and hydrogen serve as ligands.

The first example of a three-coordinate silicon compound was generated using a non-coordinating anion. Specifically, the salt [(mesityl)3Si][HCB11Me5Br6] contains a noncoordinating anion derived from a carborane. [4]

Noncoordinating anions are important components of many superacids, which result from the combination of Bronsted acids and Lewis acids.

Related Lewis acids

The neutral molecules that represent the parents to the non-coordinating anions are generally strong Lewis acids, e.g. boron trifluoride, BF3 and phosphorus pentafluoride, PF5. Perhaps the most notable Lewis acid of this genre is B(C6F5)3.[5]

References

References

  1. ↑ I. Krossing and I. Raabe (2004). “Noncoordinating Anions – Fact or Fiction? A Survey of Likely Candidates”. Angewandte Chemie International Edition. 43 (16): 2066–2090. doi:10.1002/anie.200300620.
  2. ↑ Honeychuck, R. V.; Hersh, W. H. “Coordination of “Noncoordinating” Anions: Synthesis, Characterization, and X-ray Crystal Structures of Fluorine-Bridged [SbF6]−, [BF4]−, and [PF6]− Adducts of [R3P(CO)3(NO)W]+. An Unconventional Order of Anion Donor Strength” Inorganic Chemistry 1989, volume 28, pages 2869-2886.
  3. ↑ N. A. Yakelis, R. G. Bergman (2005). “Safe Preparation and Purification of Sodium Tetrakis[(3,5-trifluoromethyl)phenyl]borate (NaBArF24): Reliable and Sensitive Analysis of Water in Solutions of Fluorinated Tetraarylborates”. Organometallics. 24: 3579–3581. doi:10.1021/om0501428.
  4. ↑ Kim, K.-C.; Reed, C. A.; Elliott, D. W.; Mueller, L. J.; Tham, F.; Lin, L.; Lambert, J. B. (2002). “Crystallographic Evidence for a Free Silylium Ion”. Science. 297: 825–827. doi:10.1126/science.1073540.
  5. ↑ Erker, G. “Tris(pentafluorophenyl)borane: a Special Boron Lewis Acid for Special Reactions”, Dalton Transactions, 2005, 1883-90.

de:Schwach koordinierende Ionen