1-Hexadecyl-2,3-dimethylimidazolium tetrafluoroborate brings a long alkyl chain together with a well-known imidazolium cation, paired with a tetrafluoroborate anion. This mouthful points to a tailored ionic liquid that often appears in chemical synthesis labs, electrochemistry projects, or specialty materials science. The chemical formula, C21H43BF4N2, shows its complexity: there’s a 16-carbon-long chain, extra methyl groups on the imidazole ring, and a fluorine-rich anion that often gives the salt its environmental stability. It looks like a waxy solid or sometimes a viscous liquid, depending on storage and temperature—a trait driven by the long hexadecyl chain. Sometimes the material appears in pale flakes or powder, or even pearl-like granules when processed under specific conditions. Its density often sits around 1.1 to 1.2 g/cm³.
The structure of this salt changes its handling in the real world. With a melting point usually between 60°C and 90°C, storage above room temperature can result in a glassy or semi-liquid state. It works well as a conductive medium, which appeals to those developing new batteries, fuel cells, or ionic liquid-based supercapacitors. The low volatility—hardly any fumes even at higher temperatures—provides real value during extended experiments. Chemical stability is another draw. Unlike many “classic” organic solvents, 1-hexadecyl-2,3-dimethylimidazolium tetrafluoroborate can handle air and humidity fairly well. That long alkyl chain bumps up hydrophobicity: it doesn’t mix easily with water but plays well with other oily or non-polar liquids. These features turn heads in solvent extraction, phase transfer catalysis, or ionic liquid lubrication—where a little stability pays dividends over time.
Imidazolium cations have been explored for decades; adding long alkyl chains and methyl groups gives even more unique combinations of surface activity and solubility. The molecular structure influences its surface tension and viscosity, which remain higher than low-molecular-weight salts—sometimes as thick as syrup. The tetrafluoroborate anion resists hydrolysis and stands up to weak acids, although strong alkali or fluorine scavengers can provoke breakdown. Laboratory batches often reach purities above 98%, with colorless to off-white appearance. Its crystalline solid form usually comes from careful, slow crystallization—fast precipitation leaves behind stickier, less manageable powder. The product’s HS Code often falls near 2933.39 (for heterocyclic compounds with nitrogen atom(s) only), reflecting its custom design and main use in specialty chemical research.
For researchers in electrochemistry, this material offers a stable, non-volatile ionic liquid that supports ionic conduction without corroding electrodes or requiring constant recycling. Those advantages trace back to its thoughtful raw materials: long-chain bromides or chlorides, imidazole, boron-based reagents, and high-purity methylation agents. The synthetic route asks for careful drying and gas protection—moisture during production can lead to hydrolysis or discoloration, which might cause downstream issues in sensitive instruments. Still, finished batches resist a lot of everyday handling, surviving weeks of storage in sealed glass bottles without degrading.
The relative safety of this material speaks to advances in modern chemistry, but no chemical arrives completely risk-free. Direct handling in large amounts can irritate skin or eyes; safe lab habits mean gloves, goggles, and using a fume hood with any open vessels. Spills clean up easily with absorbents or by scraping solids; for sticky residues, alcohols like ethanol dissolve the last traces. Disposal should always follow local regulations for fluorinated organics. Inhalation hazards stay low compared to volatile solvents, though dust from dry powder may aggravate those with existing sensitivities. The dust’s low mobility works in favor of regular lab cleaning, and the container—usually tough plastic or amber glass—protects against accidental sunlight exposure or water uptake. It’s not considered highly toxic or explosively dangerous, but the cumulative exposure over time and the fluoride content—though locked into a stable anion—means regular audits and documented inventory. Emergency guidelines and data sheets emphasize prompt washing after direct contact and immediate medical consultation if a large quantity is swallowed or splashed into eyes.
This class of ionic liquids finds a place in solid-state batteries, catalysis, and industrial processes where stability and salt tolerance count for more than mass-market price. From personal experience, the robust nature of 1-hexadecyl-2,3-dimethylimidazolium tetrafluoroborate grants confidence in small-scale organic synthesis, where other solvents might evaporate or react unpredictably before a reaction finishes up. Researchers report that using ionic liquids like this one cuts down on fire risk and cross-contamination—a lesson that stuck with me after watching colleagues experiment with classic, more volatile solvents that left a lingering smell for days. The eco-friendlier angle shows up in regulatory filings, too: low vapor pressure and the limited need for solvent exchanges reduce waste streams, provided downstream users don’t simply dump residues into drains or landfill. The hurdles—such as moderate price, specialist suppliers, or handling a dense syrup instead of crystal-clear water—don’t fade away, but they show up less often as research moves towards more tunable, safer, and longer-lasting chemical platforms in both academic and industrial labs.
