1-Hexadecyl-2,3-Dimethylimidazolium Hexafluorophosphate: Insight and Application
Historical Development
Long-chain imidazolium salts have roots in the push for novel solvents and ionic conductors. Chemists in the late 20th century began probing the effects of different alkyl substitutions on imidazolium rings with an eye on conductivity and thermal stability, especially for applications where traditional solvents fell short. Over time, lengthy alkyl chains like the hexadecyl substituent emerged, bridging research interests in surfactants, ionic liquids, and electrolyte design. The tale of 1-hexadecyl-2,3-dimethylimidazolium hexafluorophosphate traces the pathway carved by researchers seeking stable, high-performance compounds for electrochemistry, green chemistry, and material science hurdles.
Product Overview
In the world of advanced chemicals, 1-hexadecyl-2,3-dimethylimidazolium hexafluorophosphate shows up as a unique ionic liquid. Its design features a hefty hexadecyl (C16) chain paired with a rigid imidazolium core, bearing two methyl groups at the 2 and 3 positions, topped off by the famous hexafluorophosphate anion. This structure births a liquid or semi-solid material, ready for roles that demand both lipophilicity and ionic character, from surfactant work to electrolyte experimentation and catalyst design.
Physical & Chemical Properties
Density, melting range, solubility, and conductivity form the foundation for any use case. The molecule’s extended hydrocarbon chain blocks water solubility and nudges the melting point away from those of shorter-chain analogs, landing it in the soft wax to low-melting-solid bracket. It packs in thermal stability—key in high-temperature reactions. With its cationic core, the compound dispatches a high ionic conductivity in aprotic solvents, and the hexafluorophosphate anion delivers chemical robustness while steering clear of basic conditions or water hydrolysis. It comes in as an off-white waxy solid or viscous liquid, with low volatility and no significant odor.
Technical Specifications & Labeling
Producers tend to specify purity above 98%. Moisture and halide must stay minimal. The compound often carries a CAS registration—no small mark in global trade or lab research. Labels warn about hygroscopicity, flammability, and possible skin and eye irritation. Certificates of analysis detail melting points, elemental content, and spectroscopic fingerprints, which let buyers verify batch identity quickly. Containers must resist chemical attack, so high-density polyethylene or glass bottles, sealed under inert gas, have become the norm.
Preparation Method
The standard route starts from 1-hexadecylimidazole. Methylation with methyl halide (like methyl iodide) introduces the two methyl groups, often under carefully controlled temperature and solvent environments to squeeze out side reactions. Post-quaternization, metathesis swaps iodide for hexafluorophosphate. Using silver hexafluorophosphate or potassium hexafluorophosphate, chemists shake or stir the mixture in polar aprotic solvents. Filtration then removes insoluble by-products, leaving the desired salt, which is washed, dried, and sometimes recrystallized to boost purity.
Chemical Reactions & Modifications
This material shows decent chemical resilience, though strong nucleophiles or acids can break the imidazolium ring over time. Halide metathesis, alkyl substitutions, and even modifications at the alkyl tail open up chemical tuning. Some groups have explored converting the PF6⁻ anion into tetrafluoroborate, bis(trifluoromethylsulfonyl)imide, and other anions, each twisting the physical properties and expanding possible uses. The long alkyl chain also enables anchoring onto surfaces, gels, or within polymer substrates, forging new materials with blended ionic and organic characters.
Synonyms & Product Names
In catalogs, 1-hexadecyl-2,3-dimethylimidazolium hexafluorophosphate appears with several aliases. Commonly shortened as [C16C1C1Im][PF6], C16-MIMPF6, or N-hexadecyl-2,3-dimethylimidazolium hexafluorophosphate, it has gained traction in both European and North American markets under research and specialty chemical supplier brands. Some research articles lean on abbreviations or “IL” (ionic liquid) tags for clarity in text and tables.
Safety & Operational Standards
Users need to gear up with gloves, goggles, and suitable lab coats. The compound can irritate skin and mucous membranes. Inhalation is unlikely thanks to its low volatility, but dust and aerosols remain a risk during weighing or transfer. Hexafluorophosphate salts carry a hydrolysis hazard, releasing HF in contact with water or strong acids—something I learned early on in a lab job, reinforcing the need for dry conditions and properly vented spaces. Disposal must follow local guidelines, as PF6⁻ contamination carries environmental penalties in some regions. The material’s transportation usually falls under “non-hazardous” for shipping, yet still demands secure containment and spill protocols.
Application Area
My own run-ins with this compound came during electrolyte research for batteries and supercapacitors. Its long alkyl chain lines up neatly at interfaces, laying the groundwork for electric double-layer capacitance that short chains can’t match. In catalysis, this salt forms an effective reaction medium for cross-coupling and hydrogenation, taming transition metals with its unique blend of ionic and hydrophobic traits. Other labs have taken it further, stabilizing nanoparticles, coaxing proteins into solution, or spinning up anti-static coatings for electronics. Its slow interaction with water puts it in play for moisture-sensitive syntheses, separating it from shorter, more hydrophilic ionic liquids.
Research & Development
Academic and corporate research teams chase new frontiers with this compound in ionic conductivity, catalysis, lubrication, and green solvent design. Collaborations between universities and industry have pumped energy into both synthesis scale-up and property mapping. Data points show the impact of chain length on viscosity, ionic mobility, and electrochemical windows, feeding simulations and practical device development. I've watched R&D teams dissect these relationships, swapping anions and cations, blending ILs with other solvents, and targeting new environmental regulations.
Toxicity Research
Tackling toxicity, recent reports note that long-chain imidazolium salts struggle with biodegradability. The hexadecyl chain raises red flags around aquatic toxicity and membrane disruption. PF6⁻ brings its own worries, given potential HF release and environmental persistence. Cell culture studies highlight dose-dependent cytotoxicity; concentrations above low millimolar ranges can trigger cell membrane destabilization, and yet, from a practical standpoint, industrial exposures rarely cross those thresholds if procedures stick. Data gaps still exist, specifically around chronic exposure and breakdown products under real-world conditions. More eco-toxicity profiling will help shape responsible guidelines for both use and disposal.
Future Prospects
This material resides in a sweet spot for applications intersecting green chemistry, energy storage, and advanced materials. There’s growing momentum behind finding anions more benign than PF6⁻, so labs continue to rework the formula. Meanwhile, demand for safe, stable electrolytes spurs fresh investigation into blends with other ionic or molecular liquids, targeting energy density and long cycle life in new batteries. Biotechnologists watch the space, aiming to use this and similar salts for biosensor stabilization or drug delivery, provided toxicity issues get addressed. Conversation around sustainable design, safer decomposition, and full lifecycle stewardship will define the true potential—and the industries where this compound plays a central role in the years ahead.
Behind the Letters: What’s Going On With This Compound?
Breaking down the long chemical name, 1-Hexadecyl-2,3-Dimethylimidazolium Hexafluorophosphate belongs to the family of ionic liquids. That means it’s not the usual kind of liquid found in a bottle or a glass; it stands out for its unique blend of physical and chemical properties. Think of it like an oil that doesn’t vaporize easily, refuses to catch fire, and can dissolve a wide range of things other common chemicals can’t touch.
Real Uses: Shaping Laboratories and Industry
More labs keep bottles of this stuff around for one key reason: it works as a solvent and as a supporting electrolyte, especially in electrochemistry. So, researchers working on advanced batteries or sensors now have a tool that opens new doors. Compared to ordinary salts in electrochemical applications, 1-Hexadecyl-2,3-Dimethylimidazolium Hexafluorophosphate offers a larger “electrochemical window.” Sounds technical, but it means you get reactions that push performance further without breaking down. Batteries last longer. Sensors measure more precisely.
Beyond the lab, some manufacturing processes turn to this ionic liquid for its cleaning power and stability. In certain cases, it takes part in cleaning or surface treatment jobs for electronics and chip manufacturing. With all the strict rules around environmental responsibility, companies feel pressure to leave behind old solvents that pollute water or threaten workers’ health. These safer, less volatile liquids form a solution.
Environmental and Health Angle
Traditional solvents usually vanish into the air or slip into water systems, posing risks for people and the environment. Ionic liquids like this one barely evaporate. Fumes stay out of your nose and lungs. Yet, nothing’s perfect. Some studies point out that waste handling can matter just as much. If companies dump the leftovers in the wrong place or ignore disposal routines, the supposed advantage shrinks.
Regulatory voices call for tight management and tracking of chemicals like 1-Hexadecyl-2,3-Dimethylimidazolium Hexafluorophosphate. Safety data from labs and manufacturers back this up with toxicity profiles and handling instructions. In my own research experience, an emphasis on glove use, goggle use, and detailed logs becomes second nature once you see just how persistent some modern chemicals can be. It makes sense. Respect the substance, and it serves its purpose well.
Paths Forward: Making Good Ideas Work
Solvents shape industry and research. It’s not just chemists in labs but everyone who relies on smarter batteries, efficient electronics, or greener industrial processes. Chasing the next generation of safer, more capable chemicals demands real follow-through. Proper disposal, transparent testing, and continued green chemistry investments allow the benefits of ionic liquids like 1-Hexadecyl-2,3-Dimethylimidazolium Hexafluorophosphate to outweigh their drawbacks.
Manufacturers who invest in employee training and equipment design help make sure these materials never become a hazard. Honest communication about risks and ongoing study keeps the public and policymakers on board. Good science delivers answers, but thoughtful stewardship of chemicals ensures progress doesn’t stop at the lab bench.
References:- Wasserscheid, P., & Welton, T. (2007). Ionic Liquids in Synthesis. John Wiley & Sons.
- U.S. Environmental Protection Agency. Safer Choice: About Safer Chemicals.
- Journal of Physical Chemistry B, studies on ionic liquid applications and toxicity.
Why Storage Details Matter in the Lab
Every scientist knows that chemistry doesn’t stop when the experiment ends. The bottle on the shelf tells its own story. I’ve seen good compounds go to waste just because someone left the lid loose, or parked the container under a sunny window. Mistakes like that cost money and time, but sometimes the consequences turn serious, risking health or safety.
Most chemicals don’t shout warnings when they start degrading. Color might fade or clumps appear, but many shifts fly under the radar. I remember a case with an old reagent—it didn’t just underperform, it gave off fumes. All because it sat above a radiator during winter break.
Simple Steps Matter Most
Solid, basic practices go a long way. A cool, dry, well-ventilated spot usually works for a range of compounds, but temperature swings and moisture get overlooked way too often. Organic compounds, for example, tend to absorb water from the air. I’ve seen entire batches tossed because a powder turned sticky—no need for complicated instruments, just careless storage.
Never underestimate the role of sunlight. Light exposure can trigger breakdowns in photosensitive chemicals. Back in graduate school, our group lost a week’s effort after a sensitive compound turned brown on a sunny windowsill. Since then, amber bottles and opaque cabinets have become a fixture in my workspace.
Desiccators are the unsung heroes for moisture-sensitive materials. One mentor insisted on throwing in silica gel packets, even when the lab budget was tight. Seems basic, but pulling the right conditions keeps both costs and headaches down.
Label Everything and Keep It Organized
Sharp labeling isn’t just about good habits; it’s essential when tracking expiration and batch number. Missing or old labels become a guessing game in busy labs. Taking a minute to record the open date has saved me more than once.
An organized storage area also makes a big difference in day-to-day work. There’s less chance of contamination or grabbing the wrong bottle. I’ve seen mixed-up acids and bases melt through storage shelves, and nobody wants to deal with that cleanup.
Safety Goes Beyond the Basics
Some compounds demand unique precautions. Think flammables, oxidizers, explosives. These never belong near heat sources or with incompatible chemicals—rusty shelf dividers invited disaster in a local research lab not long ago. Proper flammable cabinets aren’t just regulatory checkboxes. Chemicals get hot in a standard metal cabinet, which can accelerate dangerous reactions.
Explosives and peroxides call for shorter shelf lives and regular checks for crystal buildup. Routine inspection isn’t a chore; it’s a chance to spot changes before risks grow.
Keeping Storage Smart and Safe
Good storage habits don’t require fancy technology. The smartest move is to know the properties of each compound before stocking the shelf. Read the safety datasheet carefully—it spells out what temperature and humidity ranges are safe, and flags up any dangers.
Chemical stewardship isn’t just regulation. It saves resources, prevents injuries, and keeps research rolling. Every container tells a part of the lab’s story. Handling them with care and respect ensures science progresses without setbacks, and everyone goes home safe at the end of the day.
Understanding Risk in Everyday Materials
It’s easy to brush off safety warnings as mere paperwork, but real consequences come from ignoring them. Maybe you’ve seen a Household Hazardous Waste site in your town. From batteries to cleaning sprays, certain items can spark, burn skin, or release fumes. Take bleach: mixing it with vinegar can fill your kitchen with chlorine gas, toxic enough to require evacuation. Not all risks are this dramatic, but small mistakes add up over time. People get used to using chemicals casually. A friend of mine, who worked in facilities, once rubbed his eyes after handling solvent wipes—result: lost his sight for two days. Everyday products can do real harm when they’re not handled right.
Details Matter with Chemicals
Labels aren’t decoration. They tell you what might happen if you misuse something: skin burns, lung damage, the possibility of fire. Even things that smell harmless, like ammonia or paint thinners, can be dangerous. Inhaling fumes in a closed space leads to dizziness or headaches, and it doesn’t take a big event to land someone in the ER. I know folks who have ended up with rashes after planting without gloves, just because the fertilizer label didn’t look alarming. You can’t always tell by smell or sight if something’s safe. Take time to read storage instructions—like keeping products out of the sun or away from water, since some chemicals break down and release toxic gases when damp. Changes in weather, like extreme heat, can change how products act, making explosions or leaks much more likely.
Personal Experience With “Everyday” Hazards
One summer at my first job, moving old pesticide containers, I learned fast. Metal drums had been left outdoors for years; rainwater mixed in, forming sludge. We had gloves, but no respirators. Once the lids cracked open, a thick sour smell poured out. My coworker started coughing and had to step back for air. Management assumed nothing would happen because the barrels were old, but rules matter no matter how long something’s been stored. From that point, I always looked for proper gear and open-air workspaces before tackling hazardous materials. Stories in construction and labs sound dramatic, yet most injuries are silent—chemical burns appearing hours later, lungs irritated after an afternoon in a musty shed.
What Makes a Safety Step Actually Work?
Relying on experience helps, but science and clear information go much further. Product manufacturers share safety data sheets with instructions for handling, first aid, and disposal. I always recommend wearing gloves and goggles, even if the job looks harmless. Power tools and sealed containers deserve respect. Open windows, use fans, and keep a supply of clean water nearby in any risky setting. The urge to finish fast works against safety, so slow down and check twice before mixing or disposing.
Safer alternatives are available for many old-school chemicals. Vinegar and baking soda substitute for a lot of cleaning jobs. LED bulbs have removed most mercury from homes. Ask your local recycling folks for updated disposal rules so you’re not tossing dangerous materials with regular trash. Training sessions make a difference—even seasoned workers forget basics like label checks and clean-up steps. Using your gut and the right gear turns routine jobs into safer ones for everyone involved. Houses, schools, workshops—every space benefits from solid habits around risk, not luck.
Solubility and Why It Matters
Solubility drives a lot of decisions around chemicals like 1-Hexadecyl-2,3-Dimethylimidazolium Hexafluorophosphate. Anyone dealing with this compound—chemists in research, lab techs, or industry engineers—has run into the challenge: How do you get it to dissolve, and in what? People underestimate how much time is spent just coaxing stubborn salts into solutions.
With an imidazolium ring, two methyl groups sticking out at the 2 and 3 positions, and a hefty hexadecyl chain thrown in, you aren't looking at your regular water-loving molecule. Tack on the hexafluorophosphate part and you get something sitting squarely in the camp of ionic liquids. These salts pull attention thanks to their melting points, but anyone handling them quickly learns they don’t always mix well with water.
Water Solubility: Low and Unforgiving
Here’s the simple truth: You won’t get much of this chemical to dissolve in water. That long hydrocarbon tail drags the molecule far away from anything hydrophilic. The imidazolium “head” does play well with polar environments, but the sixteen-carbon chain kills any hope of reasonable water solubility. Look up published data—solubility sits down at the limit of detection. You might get traces to dissolve with aggressive stirring or ultrasonication, but the result leaves most applications in water out of reach.
I struggled in the lab as a grad student trying to make a fine dispersion for an ionic liquid application. Even after heating and throwing in a co-solvent, visible clouds floated through the mix. Water refuses to play ball with long-chain imidazoliums, and you can forget about reliable, reproducible results when using water alone.
Solubility in Organic Solvents
Switch to organic solvents—here, things look brighter. You start to see this salt open up in solvents like acetonitrile, acetone, dichloromethane, and even ethanol. Solubility rises, and you get clear solutions at moderate concentrations. The nonpolar stretches let the compound snuggle into organic environments. Acetonitrile shows up often as a solvent in published papers because it balances the need for enough polarity to handle the charged “head” without getting bogged down by the long alkyl “tail.”
Switching solvents means you can tap into the merits of this ionic liquid in catalysis, extraction, or electrochemistry. In my own work on electrochemical cells, using acetonitrile meant all the ionic liquid went into solution, and measurements stabilized. Waste cleanup got easier, and control over experimental conditions improved.
Practical Takeaways and Solutions
If you hit a wall with solubility in one solvent, switch to a mixture. Tetrahydrofuran with a splash of DMSO works wonders for some ionic liquids. Some researchers choose alkyl-chain “tuning”—they chop down the hydrocarbon length for better water compatibility, but lose hydrophobic interactions that some applications want. It all comes down to compromise.
Handling this compound highlights the value of going back to basics: look at the structure, run small-scale solubility tests, and keep detailed notes. That habit serves better in the long run than relying solely on published tables. Companies that use these salts for battery tech, organic transformations, or as extraction agents often factor in cost, waste management, and process safety tied directly to solvent choice.
In the end, solubility rules shape what’s practical on the bench or the plant floor. Knowing your compound ensures less time frustrated at cloudy mixtures—and more time focusing on experimental results.
Recognizing the Risks That Come With Chemicals
Walking into a lab or factory, you spot a drum sitting in the corner—label faded, but you can just make out something about “irritant” or “corrosive.” That’s not just fine print. Anyone who’s worked with chemicals learns early how a little exposure can turn into a nasty situation. According to the National Institute for Occupational Safety and Health, over 190,000 illnesses and injuries each year come from workplace chemical exposures in the United States. The consequences can go from mild rashes to severe burns, lung injuries, or even cancer.
Basic Principles—No Shortcuts
Each chemical brings its own hazards. An acid splash won’t give you much warning before you feel it. Vapors from solvents don’t always smell strong to start, but can sting your lungs and eyes. Relying on memory or rumors about what’s “safe enough” just stacks the odds against your health.
Manufacturers legally provide Safety Data Sheets, and these are worth reading. They don’t just list the dangers—they tell you what actually stops harm. Looking up the SDS gives you important details, like which gloves, respirators, or goggles block risks. Nitrile gloves might hold up against many solvents, but not all. Acids often break through latex. A dust mask won’t stop fumes from heavy-duty cleaners; a respirator with the right cartridge will.
What Works and Why—Experience Talks
Years ago, I watched a co-worker try to handle a drum of phosphoric acid with nothing but cotton gloves and hope. The gloves dissolved in fifteen minutes. After a trip to the clinic for chemical burns, nobody doubted the point of the thick rubber gloves and face shields. Mother Nature and chemistry don’t care about shortcuts or tight schedules.
For splashes, chemical-resistant goggles and full face shields become regular gear. Half-tucking goggles in your bag for next time never keeps eyes safe. Disposable chemical suits can look bulky, but after seeing skin reactions from missed drips, I stopped noticing how awkward they felt. Proper ventilation—a simple exhaust hood—has kept me conscious a few times when cleaning vapor-heavy equipment.
Culture and Commitment: Every Level Counts
Creating rules and stocking equipment isn’t enough by itself. People mimic what they see. If the manager skips the gloves, the new hire will likely follow. Teams that take a few minutes to explain why equipment matters and show how to use it right tend to work more confidently—and get hurt less. The difference I’ve seen between labs with a “just get it done” mindset and those that treat safety as part of the day is night and day in injury rates.
Solid Steps for Real Protection
In my experience, the best results come from combining solid information with accessible protective gear and ongoing training. Make the right gloves easy to grab. Post instructions at every station on what to wear and why. Practice what to do if something does spill so panic doesn’t win the day. Report faulty gear or empty soap dispensers as soon as you spot them—don’t cross your fingers and hope for the best.
Working with chemicals never goes on autopilot. Getting home safe means taking a few moments to suit up and double-check labels—both your health and the health of your coworkers depend on it.
