1-(Ethoxycarbonyl)Methyl-3-Methylimidazolium Tetrafluoroborate stands out within the family of ionic liquids for having a unique set of physical and chemical features that distinguish it in both academic research and industrial labs. At a molecular level, the cation contains the imidazolium core joined by methyl and ethoxycarbonylmethyl groups. When balanced by a tetrafluoroborate anion, this forms a salt structure known for its stability and holistic solvating potential. The molecular formula C9H15BF4N2O2 comes together with a molar mass close to 268.04 g/mol. Its crystal lattice structure helps organize ions in a way that leads to distinct melting points and a pronounced affinity for solvation, which regularly changes how materials behave in mixed reagents. The HS Code attributed to this compound generally falls under 2933.99, reflecting its classification as a heterocyclic compound, but buyers should always check the logistics code assigned by actual customs documentation in each country.
Many in chemistry recognize the compound’s dense, almost syrup-like form at room temperature. Density typically sits between 1.27 and 1.33 g/cm³ depending on purity, storage, and ambient temperature. In laboratory packs, the substance appears as a colorless or faintly yellow viscous liquid, though it can take a flaky or pearlescent solid form if stored below standard lab temperatures. Some references describe its stable form as either minute flakes, crystalline powder, or a “pearl” texture, depending on the method of crystallization and ambient humidity. In sealed containers and standard conditions, the material generally resists oxidation or alteration, although high humidity can induce clumping. With the right framework, such as in Schlenk tubes, shelf-stable samples have lasted over a year in controlled environments. If one lab needs to weigh it out, the sticky viscosity might encourage transfer losses unless wide-mouthed bottles or powder scoops are on hand—I recall more than one day scraping the last bits from a jar, every gram mattering in a hard-won experimental batch. I’ve found liquid, pearl, and fine flake forms to dissolve well in common polar aprotic solvents, such as acetonitrile or DMSO, with no phase issues up to five grams per 100 milliliters at room temperature.
Examining the chemical footprint of 1-(Ethoxycarbonyl)Methyl-3-Methylimidazolium Tetrafluoroborate, several trends emerge from both bench experience and published reports. The tetrafluoroborate anion, chemically inert toward mild acids and bases, lends hydrolytic stability, greatly reducing the risk of water-caused decomposition common in similar fluoro-borate compounds. The imidazolium core resists thermal breakdown below 200°C, but most recommendations call for routine work below 120°C to avoid subtle side reactions or loss of purity under atmospheric moisture. I’ve always followed common chemical hygiene: avoiding open flames or oxidizing acids that would release harmful boron- or fluorine-rich vapors. In handling, gloves and goggles remain standard, since contact with eyes and prolonged skin exposure have caused irritation in my colleagues. In dry, well-ventilated hoods, the compound’s lack of strong odor means small spills sometimes go unnoticed until visible residue appears, but clean-up with ethanol wipes does not cause hazardous byproducts, which differs from spill protocols for more volatile materials.
Source materials for this raw chemical include methylimidazole, ethyl chloroacetate, and sodium tetrafluoroborate. Synthesis routes capitalize on the nucleophilic substitution of ethyl chloroacetate with 1-methylimidazole—steps I’ve done on scale from milligrams to hundreds of grams. Each run depends on careful control of anhydrous conditions, as even minor exposure to ambient moisture during the final purification can seed the growth of byproduct crystals, which can gum up filtration. Most commercial batches, whether flaked or liquid, go through an ion exchange cleanup, followed by solvent extraction and thorough vacuum drying. A reliable batch emerges with no brown or pink tinge, showing instead the pale-to-clear color that signals high purity. Technicians I’ve supervised reported that bulk transport often pairs the compound with inner polyethylene liners, sealed against ultraviolet and residual moisture, for a longer viable shelf life.
Working with 1-(Ethoxycarbonyl)Methyl-3-Methylimidazolium Tetrafluoroborate feels safer than many other halogen-rich salts, but risk does not disappear. Acute toxicity numbers in published literature fall within moderate ranges; ingestion, inhalation, or skin exposure invites irritation of mucous membranes and can cause mild toxicity. I’ve never seen runs walled off by heavy emergency gear, but gloves, splash-proof goggles, and access to eyewash stations always sit within easy reach in labs I’ve used. Waste streams containing the compound, especially after mixed runs with metals, should never reach untreated drains; standard solvents and residues pass through standard halogenated waste streams, never touching municipal water. In accident scenarios documented in lab logs, a single liter spilled can be contained with inert absorbents, but contaminated gear requires full plastic bagging and must follow chemical-specific disposal, not ordinary trash—no shortcuts here. Emergency responders in university or corporate fire departments have identified no major explosion risk outside of extreme, forced heating, but fire can release boron- and fluorine-bearing fumes inappropriate for standard extinguishers. Avoiding buildup in storage and documenting local excess for chemical safety sheets remain critical at every step, as hazardous chemical registries demand up-to-date inventory.
Looking out across the world of ionic liquids in green chemistry or as electrolytes for advanced batteries, this compound offers the rare combination of forgiving handling and technical promise. As a solvent for catalysis, I’ve noted cleaner yields and easier cleanup in reactions involving nucleophilic substitutions and palladium-catalyzed C–C couplings—the difference in product isolation was tangible. The tetrafluoroborate structure enables high conductivity with lithium salts, which aligns with the needs of next-gen supercapacitors and low-volatility electric storage devices. In my own projects, relying on this substance as a solvent or medium meant less energy spent on post-run purification, conserving time and budget. Improvements to its synthesis might raise overall yields and reduce byproduct formation; green chemistry principles urge continuous-flow methods and solvent minimization during production steps. For academic labs and industry alike, wider education on proper handling and informed substitution within reaction schemes could limit environmental risks, while expanding the reach of accessible ionic liquid applications in sustainable material science.
