Non-coordinating anion
Anions that interact weakly with cations are 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). 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. Noncoordinating anions are important components of many superacids, which result from the combination of Bronsted acids and Lewis acids.
Contents
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] 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, such as triflates were considered to be low-coordinating with some cations.
Era of BARF
A revolution in this area occurred in the 1990s with the introduction of the [B[3,5-(CF3)2C6H3]4]− anion, commonly abbreviated as [BArF4]− and affectionately called "BARF."[3]. This anion is far less coordinating than the tetrafluoroborate BF4−, hexafluorophosphate PF6−, and perchlorate ClO4−, and consequently has enabled the study of still more electrophilic cations.[4]
In the tetraarylborates, the negative charge is symmetrically distributed over many electronegative atoms. Related anions are derived from tris(pentafluorophenyl)boron B(C6F5)3. 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.
The first preparation of B[3,5-(CF3)2C6H3]4− was reported by Kobayashi and co-workers; for that reason, it is sometimes referred to as Kobayashi's anion.[5] This method of preparation has been superseded by a safer route.[3]
Other types of non-coordinating anions
A second major class of non-coordinating anions are derived from carboranes. For example, the first example of a three-coordinate silicon compound, the salt [(mesityl)3Si][HCB11Me5Br6] contains a noncoordinating anion derived from a carborane. [6]
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.[7], tris(pentafluorophenyl)borane.
References
Cite error: Invalid <references> tag;
parameter "group" is allowed only.
<references />, or <references group="..." />de:Schwach koordinierende Ionen
- ↑ 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. PMID 15083452.
- ↑ Honeychuck, R. V.; Hersh, W. H. (1989). "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. 28 (14): 2869–2886. doi:10.1021/ic00313a034.
- ↑ 3.0 3.1 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 (14): 3579–3581. doi:10.1021/om0501428. PMC 2600718 Freely accessible. PMID 19079785.
- ↑ M. Brookhart, B. Grant, A. F. Volpe, Jr. (1992). "[(3,5-(CF3)2C6H3)4B]-[H(OEt2)2]+: a convenient reagent for generation and stabilization of cationic, highly electrophilic organometallic complexes". Organometallics. 11: 3920–3922. doi:10.1021/om00059a071.
- ↑ H. Nishida, N. Takada, M. Yoshimura, T. Sonods, H. Kobayshi (1984). "Tetrakis(3,5-bis(trifluoromethyl)phenyl)borate. Highly lipophilic stable anionic agent for solvent-extraction of cations". Bulletin of the Chemical Society of Japan. 57: 2600. doi:10.1246/bcsj.57.2600.
- ↑ 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 (5582): 825–827. doi:10.1126/science.1073540. PMID 12161650.
- ↑ G.Erker (2005). "Tris(pentafluorophenyl)borane: a Special Boron Lewis Acid for Special Reactions". Dalton Transactions (11): 1883–1890. doi:10.1039/b503688g. PMID 15909033.
