Transition metal chloride - Inorganic chloride salt - Inorganic salt
Descrizione
This compound belongs to the class of inorganic compounds known as transition metal chlorides. These are inorganic compounds in which the largest halogen atom is Chlorine, and the heaviest metal atom is a transition metal.
External Descriptors
ammonium salt
1. Djoumbou Feunang Y, Eisner R, Knox C, Chepelev L, Hastings J, Owen G, Fahy E, Steinbeck C, Subramanian S, Bolton E, Greiner R, and Wishart DS. ClassyFire: Automated Chemical Classification With A Comprehensive, Computable Taxonomy. Journal of Cheminformatics, 2016, 8:61.
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Recensioni
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Application Protocols
No assay or immunoapplication protocols apply to this inorganic salt.
General lab protocol examples (literature/general)
Preparing an aqueous stock: Dissolve the solid in deionized water containing a small amount of HCl (e.g., 1–10 mM) to maintain chloride activity. Filter through 0.2 µm if particle-free solutions are required.
Nanoparticle synthesis setup: Charge a reactor with polyol solvent and stabilizer (e.g., PVP), heat under N2, then add the aqueous iridium solution dropwise while sparging with N2 or H2; quench growth by cooling and diluting.
These are general research suggestions only; adapt and validate for your specific application.
Biological Roles
This product is an inorganic iridium coordination salt used primarily in materials and synthetic chemistry. It does not serve a physiological role and is not intended for biological systems.
General notes (literature/general)
Iridium is not an essential biological element; soluble iridium salts may interact nonspecifically with proteins and nucleic acids due to charge and ligand exchange, but such interactions are not considered biological functions.
Certain iridium complexes have been studied as probes or catalysts in chemical biology; however, those applications typically use specifically designed organometallic complexes rather than simple hexachloroiridate salts.
Research Use Only
As stated by the manufacturer: For research use only. Not for diagnostic, therapeutic, or clinical use.
Buffer Applications
Not typically applicable. Ammonium hexachloroiridate-type salts are not used as buffering agents and do not constitute a defined buffer system.
Practical note
If aqueous work is required, maintain chloride activity (e.g., add NaCl or a small amount of HCl) rather than using common biological buffers that can coordinate or raise pH, which promotes hydrolysis/substitution.
Avoid amine-containing buffering agents (e.g., Tris) if preserving the chloride coordination sphere is important, as such ligands may substitute at iridium.
Green Alternatives
Context
Iridium salts are critical for high-performance catalysis and electrochemistry; however, iridium is rare and energy-intensive to refine. Greener practice emphasizes minimization, recycling, and avoidance where possible.
Greener choices and strategies (literature/general)
Metal minimization: Employ lower catalyst loadings via improved dispersion (e.g., nanoparticle supports, single-atom catalysts) to reduce total Ir usage.
Alternative precursors: Where chloride is problematic (e.g., corrosion, waste streams), nitrate- or acetate-based Ir precursors can simplify wastewater treatment, though they may be less stable.
Solvent choices: Favor water or benign polyols for reductions instead of high-boiling toxic solvents; avoid strongly coordinating aprotics when unnecessary.
Recovery/recycling: Implement ion-exchange or electrodeposition to recover iridium from mother liquors and spent catalysts; close-loop metal recovery has the largest sustainability impact.
Process intensification: Flow reduction processes in aqueous media can improve safety and heat/mass transfer while reducing solvent volumes.
Trade-offs
Chloride complexes provide stability and synthetic control; moving to non-chloride precursors may increase sensitivity to hydrolysis or change nucleation behavior.
Water-based systems are greener but can complicate ligand control and particle monodispersity; additives (Cl−, buffers, benign stabilizers) may be required.
Comparison snapshot (general)
[IrCl6]2− vs Ir nitrate: Chloride precursor offers higher stability in acidic media; nitrate variant eases Cl−-free downstream processing but may hydrolyze more readily.
Pharmaceutical Uses
Not applicable to this product class. This item is not an excipient and is not used for human or veterinary formulation.
Manufacturing context (general)
In pharmaceutical process development, iridium salts occasionally appear as research catalysts for challenging transformations; however, such uses are confined to R&D, and residual iridium is rigorously removed. This product is supplied strictly for research use only.
Regulatory note
No pharmacopeial monograph is associated with ammonium hexachloroiridate salts to the best of general knowledge. Confirm any regulatory requirements independently if considering process-development use.
Physical Properties
Item-specific physical specifications have not been provided for this SKU; consult the CoA/Spec Sheet for authoritative values.
Item-specific properties
Appearance: Not specified for this item; refer to CoA/Spec Sheet.
Density: Not specified for this item; refer to CoA/Spec Sheet.
Melting/Decomposition point: Not specified for this item; refer to CoA/Spec Sheet.
Solubility: Not specified for this item; refer to CoA/Spec Sheet.
UV-Vis cutoff/absorbance: Not specified for this item; refer to CoA/Spec Sheet.
Literature/general properties for (NH4)2[IrCl6]
Phase: Ionic inorganic solid; typically forms crystalline powders.
Thermal behavior: Tends to decompose on strong heating rather than exhibit a sharp melt; decomposition may produce HCl/Cl-containing fumes and Ir metal/oxides (literature/general).
Solubility profile: Generally soluble in water; limited solubility in most nonpolar organic solvents. Hydrolysis can occur in basic aqueous media with ligand substitution by hydroxide (literature/general).
Color: Frequently reported as yellow–orange to red crystals for hexachloroiridate(IV) salts, depending on hydration and crystal habit (literature/general).
Magnetic/optical: Low-spin d4 complex; characteristic ligand-to-metal charge-transfer bands in the visible can impart color (literature/general).
Computed/estimation notes
LogP, pKa, refractive index are not meaningful for this ionic coordination salt in the conventional sense; values are not typically reported.
Always verify item-specific data from the product CoA; do not rely on general literature values for critical specifications.
Quality and Grades
Item-specific grade/purity: Not specified for this item; refer to CoA/Spec Sheet.
What the grade typically implies (general guidance)
Research grade inorganic salts are suitable for most synthetic, materials, and analytical workflows. If labeled as high-purity or trace-metal grade, they are often screened for very low levels of metallic contaminants that could interfere with catalysis or nanomaterials synthesis.
For spectroscopy/HPLC designations (less common for this class), lower UV absorbance and controlled water/halide impurity levels would be expected and documented on the CoA.
Stabilizers/additives
Stabilizer content: Not specified for this item; refer to CoA/Spec Sheet.
Many chloride complexes are supplied neat with no stabilizer; moisture control is usually sufficient to preserve integrity. If hydration state is relevant, it will be called out on the CoA.
Practical guidance for this product class
If the material is used as a precursor for iridium nanoparticles or as a catalyst precursor, trace metal impurities (Pt, Pd, Fe, Cu) and residual nitrate/sulfate can influence nucleation and catalytic performance. Request impurity profiling if critical to your application.
If solid-state or optical studies are planned, confirm the oxidation state (Ir(IV) vs Ir(III)), hydration level, and chloride content via the CoA; these affect color, spectral features, and reactivity.
Always rely on the provided CoA/Spec Sheet for item-specific specifications, tests, and acceptance criteria.
Reaction and Applications
Materials synthesis (literature/general)
Precursor for iridium metal nanoparticles via chemical reduction (e.g., H2, NaBH4, alcohol/polyol) with applications in hydrogenation, dehydrogenation, and electrocatalysis (OER/ORR when converted to Ir/IrO2).
Starting material for IrO2 formation by thermal or oxidative treatments; IrO2 is widely used in electrochemical anodes and as a robust catalyst support.
Anion metathesis route to alternative iridium complexes: Exchange Cl− with other ligands (CN−, N-donors, phosphines) via stepwise substitution, often proceeding through aquo intermediates under controlled conditions.
Coordination and redox chemistry (literature/general)
The [IrCl6]2− anion (Ir(IV), d4 low-spin) undergoes ligand substitution (aquation) in water; substitution rates accelerate with heat and lower [Cl−].
Redox-active: Readily reduced to Ir(III) or Ir(0) by common reducing agents; oxidation to higher states requires strong oxidants.
Practical tips
Maintain chloride activity (e.g., 0.1–1 M NaCl/HCl) to suppress undesired ligand exchange when isolating chloride-rich species.
Degas solutions and exclude adventitious base if oxidation state control is important.
For nanoparticle syntheses, seed-mediated growth and surfactant/stabilizer choice (e.g., PVP, citrate) dramatically impact dispersion and facet control.
Analytical uses (literature/general)
Can serve as a standard/starting point in kinetic studies of ligand substitution and electron-transfer processes of octahedral Ir complexes.
Manufacturer Applications: Not specified for this item; users typically employ this salt as an iridium precursor in materials science workflows.
Reaction Conditions
The following are representative literature conditions for typical transformations starting from ammonium hexachloroiridate-type salts; they are general guidance and not specifications for this item.
Reduction to Ir(0) nanoparticles (literature/general)
Solvent: Ethylene glycol (polyol) or water/alcohol mixtures.
Reductant: NaBH4 (0–5 °C to room temperature) or H2 (1–10 bar) at 50–150 °C.
Additives: PVP, citrate, or Cl− to control nucleation and growth; inert atmosphere recommended.
Outcome: Ir nanoparticles (2–5 nm typical) with size tunable by reductant rate and ligand coverage.
Formation of IrO2 (literature/general)
Route A: Thermal decomposition/calcination of dried precursor on support under air/O2 at 350–500 °C.
Route B: Wet-chemical oxidation with peroxides followed by annealing; pH control avoids excessive hydrolysis.
Ligand substitution/aquation (literature/general)
Medium: Aqueous HCl to suppress aquation; to induce substitution, reduce [Cl−] and heat (50–90 °C) to generate aqua/hydroxo intermediates, then introduce target ligands (e.g., bpy, phen, phosphines) under inert conditions.
Redox step: If Ir(III) complexes are desired, include a mild reductant (ascorbate, sulfite) during or after substitution.
Workup and purification
Avoid strong bases; neutralize carefully after reactions involving HCl. Precipitate with non-coordinating anions (PF6−/BF4−) when needed to isolate neutral complexes.
Verify and optimize conditions experimentally for your system.
Safety and Handling
Safety classifications for this specific lot are not provided here. Always consult the product SDS for definitive hazard, first-aid, and regulatory information.
GHS information (item-specific)
Signal word, hazard statements, pictograms, and GHS classification: Not specified for this item; refer to SDS.
General hazards for hexachloroiridate salts (literature/general)
May cause irritation to skin, eyes, and respiratory tract upon contact or inhalation of dust.
Harmful if swallowed; heavy-metal salts may present systemic toxicity if ingested.
Environmental hazard: Transition-metal chlorocomplexes should be prevented from entering waterways; dispose as hazardous waste per local regulations.
Handling recommendations
Use in a fume hood to control dust and potential HCl-containing fumes if heated.
PPE: Lab coat, safety glasses or face shield, and appropriate chemically resistant gloves (e.g., nitrile). Avoid skin contact and inhalation of dust/aerosols.
Incompatibilities: Strong reducing agents (may reduce Ir(IV) to Ir(III)/Ir(0) with release of chloride); strong bases (hydrolysis/substitution to hydroxo species); strong acids with oxidants may evolve chlorine-containing gases; avoid contact with finely divided reactive metals.
First-aid overview (general)
Skin/eye contact: Rinse with water for at least 15 min; remove contaminated clothing; seek medical evaluation.
Inhalation: Move to fresh air; seek medical attention if symptoms persist.
Ingestion: Rinse mouth; do not induce vomiting; seek medical attention.
Store tightly closed, desiccated, at room temperature as specified for this item. Defer to SDS for spill response and firefighting guidance.
Solvent Selection
This compound is an ionic iridium chlorocomplex salt; solvent choice primarily governs hydrolysis, ligand exchange, and reduction behavior.
Polarity/miscibility (literature/general)
Water: Typically soluble; solutions are acidic to mildly acidic due to ammonium and chloride. Hydrolysis occurs under basic conditions.
Alcohols (MeOH, EtOH, iPrOH): Limited solubility; solubility may improve with added chloride (e.g., HCl) to suppress hydrolysis.
Polar aprotics (DMSO, DMF): Variable behavior; coordination and ligand substitution may occur. Exercise caution if the intact [IrCl6]2− complex is required.
Nonpolar solvents (hexanes, toluene, ethers): Essentially insoluble; use biphasic or phase-transfer strategies if needed.
Practical selection tips
To preserve the hexachloroiridate(IV) anion, use chloride-rich, mildly acidic aqueous media (e.g., water with a small amount of HCl) to minimize aquation or hydroxo formation (literature/general).
For nanoparticle synthesis via polyol or alcoholic reduction, premixing aqueous solutions into hot ethylene glycol or polyol media can be effective; maintain chloride concentration to control nucleation.
Avoid strongly basic or strongly coordinating solvents if oxidation state/ligand integrity is critical.
Comparison (general)
Hexachloroiridate salts vs nitrate/sulfate iridium salts: Chloride complexes are more resistant to uncontrolled hydrolysis in acidic media and convenient for anion metathesis. Nitrate salts may be preferred where chloride contamination must be avoided (e.g., certain electrocatalyst preparations).
Storage and Reconstitution
Storage (item-specific)
Storage conditions: Room temperature, Desiccated (as provided in Product Data).
Shipped in: Normal conditions.
Container: Keep tightly closed in a dry, well-ventilated place. Protect from prolonged exposure to humidity.
Stability considerations (general)
Moisture and basic conditions promote hydrolysis/ligand exchange; maintain dry storage and avoid residual base contamination.
Avoid contact with strong reducing agents during storage.
Reconstitution and solution handling (general)
Solvent: Use deionized water; to preserve the chloride coordination sphere, include a small amount of HCl or NaCl (e.g., 1–100 mM depending on application).
Filtration: If clarity is required, filter through 0.2 µm PTFE or PES. Avoid cellulose nitrate if using acidic solutions that may leach contaminants.
Working solutions: Prepare fresh when possible. If short-term storage is needed, keep solutions at 2–8 °C in the dark and in glass or compatible polymer; monitor for precipitation or color change.
Shelf-life
Not specified for this item; refer to CoA/Spec Sheet.
Always consult the product CoA and SDS for definitive guidance on storage stability and safe handling of solutions. For research use only.
Structure and Identity
Ammonium chloroiride (CAS 16940-92-4) is best known in the literature as the hexachloroiridate(IV) ammonium salt, typically formulated as (NH4)2[IrCl6], a classical octahedral Ir(IV) coordination complex used in materials and catalysis research.
Item-specific identifiers
SKU: A113306
CAS: 16940-92-4
InChIKey (as provided): 211026
SMILES (item-specific): Not specified for this item; refer to CoA/Spec Sheet.
Chemical name on label: Ammonium chloroiride (catalog naming)
Structural features (literature/general)
Likely composition: (NH4)2[IrCl6] (hexachloroiridate(IV) dianion charge-balanced by two ammonium cations)
Coordination environment: Iridium(IV) in an octahedral field coordinated by six chloride ligands; the [IrCl6]2− anion is typically low-spin d4.
Ionic assembly: Two ammonium counter-cations engage in H-bonding to the chloride ligands in the solid state.
2D description in words: A central Ir atom surrounded octahedrally by six terminal Cl ligands (forming the [IrCl6]2− complex anion) with two NH4+ ions nearby to balance charge; no covalent bonds between anion and cations.
Empirical/molecular data (literature/general)
Molecular formula (for (NH4)2[IrCl6]): H8Cl6IrN2 (literature)
Formula weight (for (NH4)2[IrCl6]): ~441.01 g/mol (literature)
Note: The exact structural identity and stoichiometry for the supplied item should be confirmed from the product CoA/Spec Sheet.
Synthetic Utility
Precursor versatility (literature/general)
[IrCl6]2− serves as a robust, isolable Ir(IV) source. It can be selectively reduced to Ir(III) for preparation of classical Ir(III) complexes (e.g., [IrCl6]3−, [IrCl5(H2O)]2−) and further converted to cyclometalated or phosphine-ligated Ir(III) catalysts.
Chloride ligands provide a tunable platform for stepwise substitution by neutral donors (pyridines, phosphines, NHC precursors) via aquation pathways.
Materials routes
Thermal or chemical transformation to IrO2 under oxidative conditions yields a benchmark electrocatalyst for oxygen evolution. Deposition on conductive supports (e.g., Ti, FTO, carbon) can be accomplished from aqueous chloride precursors.
Reduction to Ir(0) nanoparticles enables heterogeneous catalysis in hydrogenation and dehydrogenation; particle size and dispersion are controllable through ligand/surfactant and chloride concentration.
Retrosynthetic value
Starting from a well-defined halide complex streamlines purification and stoichiometry in downstream ligand syntheses; the chloride counterion simplifies anion metathesis (e.g., to PF6−, BF4−) after coordination sphere installation.
Practical highlights
Maintain acidic, chloride-rich conditions for isolating chlorido complexes; switch to controlled base or coordinating ligands to drive substitution.
For luminescent Ir(III) complexes (e.g., OLED research), reduction from Ir(IV) chloride precursors to Ir(III) and subsequent cyclometalation is a common route.
Target Specificity
Not applicable. This product is an inorganic coordination salt, not a biological targeting reagent. No antigen, epitope, species reactivity, clone, or isotype information applies.
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