Counterion

A counterion (pronounced as two words, i.e. "counter" "ion", and sometimes written as two words) is the ion that accompanies an ionic species in order to maintain electric neutrality. In table salt (NaCl), the sodium ion (positively charged) is the counterion for the chlorine ion (negatively charged) and vice versa.

Polystyrene sulfonate, a cation exchange resin, is typically supplied with Na⁺ as the counterion.

A counterion will be more commonly referred to as an anion or a cation, depending on whether it is negatively or positively charged. Thus, the counterion to an anion will be a cation, and vice-versa.

Interfacial chemistry

Counterions are the mobile ions in ion exchange polymers and colloids.[1] Ion exchange resins are polymers with a net negative or positive charge. Cation exchange resins consist of an anionic polymer with countercations, typically Na⁺ (sodium). The resin has a higher affinity for highly charged countercations, for example by Ca²⁺ (calcium) in the case of water softening. Correspondingly, anion exchange resins are typically provided in the form of chloride Cl⁻, which is a highly mobile couteranion.

Counterions are used in phase-transfer catalysis. In a typical application lipophilic countercation such as benzalkonium solubilizes reagents in organic solvents.

Solution chemistry

Solubility of salts in organic solvents is a function of both the cation and the anion. The solubility of cations in organic solvents can be enhanced when the anion is lipophilic. Similarly, the solubility of anions in organic solvents is enhanced with lipophilic cations. The most common lipophilic cations are quaternary ammonium cations, called "quat salts".

• Lipophilic counteranions
• 
  Lithium tetrakis(pentafluorophenyl)borate is the lithium salt of a highly lipophilic tetraarylborate anion, often referred to as a weakly coordinating anion.[2]
• 
  Tetraphenylborate is less lipophilic than the perfluorinated derivative, but widely used as a precipitating agent.
• 
  Hexafluorophosphate is a common weakly coordinating anion.
• 
  As illustrated by the small counteranion tetrafluoroborate (BF⁻
  ₄), lipophilic cations tend to be symmetric and singly charged.

• Lipophilic countercations
• 
  Bis(triphenylphosphine)iminium chloride is the chloride salt of a bulky lipophilic phosphonium cation [Ph₃PNPPh₃]⁺.
• 
  Tetraphenylphosphonium chloride (C₆H₅)₄PCl, abbreviated Ph₄PCl or PPh₄Cl is the chloride of a symmetrical phosphonium cation that is often used in organometallic chemistry. The arsonium salt is also well known.
• 
  The bromide salt of tetrabutylammonium, one of the most common counter cations. Many analogous "quat salts" are known.
• 
  Alkali metal cations bound by crown ethers are common lipophilic countercations, as illustrated by [Li(12-crown-4)₂]⁺.

Many cationic organometallic complexes are isolated with inert, noncoordinating counterions. Ferrocenium tetrafluoroborate is one such example.

Electrochemistry

In order to achieve high ionic conductivity, electrochemical measurements are conducted in the presence of excess electrolyte. In water the electrolyte is often a simple salt such as potassium chloride. For measurements in nonaqueous solutions, salts composed of both lipophilic cations and anions are employed, e.g., tetrabutylammonium hexafluorophosphate. Even in such cases potentials are influenced by ion-pairing, an effect that is accentuated in solvents of low dielectric constant.[3]

Counterion stability

For many applications, the counterion simply provides charge and lipophilicity that allows manipulation of its partner ion. The counterion is expected to be chemically inert. For counteranions, inertness is expressed in terms of low Lewis basicity. The counterions are ideally rugged and unreactive. For quaternary ammonium and phosphonium countercations, inertness is related to their resistance of degradation by strong bases and strong nucleophiles.

References

1. IUPAC, Compendium of Chemical Terminology, 2nd ed. (the "Gold Book") (1997). Online corrected version:  (2006–) "counter-ions". doi:10.1351/goldbook.C01371
2. 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.
3. Geiger, W. E., Barrière, F., "Organometallic Electrochemistry Based on Electrolytes Containing Weakly-Coordinating Fluoroarylborate Anions", Acc. Chem. Res. 2010, 43, 1030. doi:10.1021/ar1000023