N-Butyl-N-Methylpyrrolidinium Iodide: A Detailed Commentary
Historical Development
Chemists have known about pyrrolidinium salts since the middle of the 20th century. The rise of N-Butyl-N-methylpyrrolidinium iodide tracked directly with the surge in interest in ionic liquids in the 1990s. Those years saw researchers dig deeper into the range of quaternized nitrogen heterocycles, all hunting for new options for electrochemical applications and green chemistry. The iodide derivative entered the spotlight as folks experimented with alkyl substitution on the pyrrolidinium ring, tweaking both physical stability and ionic conductivity. Academic groups published most of this work in journals focused on synthetic chemistry and materials research, often with a nod toward device-oriented outcomes or greener lab protocols. If you trace patents and published articles, you get a picture of a compound moving from curiosity to real prospect for battery and catalysis tech, showing just how fast some niche chemicals can gain traction when they land in the right field.
Product Overview
N-Butyl-N-methylpyrrolidinium iodide stands out as a quaternary ammonium salt, made up of a pyrrolidine ring bonded to both butyl and methyl groups, capped by an iodide anion. Solid at room temperature and packing a decent molecular weight, it offers a blend of physicochemical traits that suit it for use in next-generation electrolytes, phase transfer catalysts, and advanced materials labs. Its consistency and shelf stability stack up well against legacy ammonium salts, making it attractive to research teams who value predictable results and minimal fuss during handling or scaling up. Reliable packaging, often in amber glass bottles with moisture protection, gives both big labs and smaller outfits confidence in storage and shipping.
Physical & Chemical Properties
Most folks who’ve spent time with these pyrrolidinium salts will tell you they appreciate the powdery or sometimes crystalline solid form, which shows off solid solubility in polar solvents like water, acetonitrile, and many alcohols. The compound’s colorless or pale white appearance makes it easy to monitor during reactions. Chemically, it resists most mild oxidants, and users can count on reasonable thermal stability up toward 200°C, as long as extreme pH swings or strong reducing agents stay out of the picture. The iodide anion can sometimes serve as a nucleophile in displacement reactions, which gives a bonus route for functionalization and post-reaction transformations. Moisture and air shouldn’t bother it much, though everyone agrees dry, airtight storage makes a real difference in shelf life, especially in humid climates.
Technical Specifications & Labeling
Most suppliers provide N-Butyl-N-methylpyrrolidinium iodide at a purity above 98%, supported by HPLC or NMR validation. Labels on bottles list the CAS number and relevant hazard codes, along with recommended temperature and light protection. For most research purposes, users expect a clear certificate of analysis—listing melting range (often around 150-180°C), moisture content, and spectral data. Safety data highlights any incompatibilities, as well as recommended personal protective equipment. Labs appreciate this level of information—it saves headaches on compliance and gives techs confidence when moving from bench to pilot-scale preparation.
Preparation Method
The preparation usually kicks off from N-methylpyrrolidine, reacting with n-butyl iodide under solvent conditions that favor the SN2 pathway—typically acetonitrile or dichloromethane as the solvent, often with mild heating or overnight stirring. This method gets a reliable conversion, with organic extraction and crystallization yielding a bounty of crisp, solid iodide salt. Anyone who’s handled larger batches recognizes the persistent iodine odor and takes note of the need for solid ventilation. The approach easily adapts to larger scales with only minor tweaks to reactor size and purification setup, which has helped academic and industrial groups source plenty for ongoing electrolyte research.
Chemical Reactions & Modifications
Researchers lean on this salt for its utility as a precursor in metathesis reactions, swapping iodide for other anions—tetrafluoroborate, hexafluorophosphate, and bis(trifluoromethane)sulfonimide all get used frequently to make a range of ionic liquids. The cation itself stays remarkably stable in the face of strong bases and acids, and modifications at the butyl or methyl position happen rarely unless you take a sledgehammer approach with aggressive alkyl radicals or UV irradiation. In catalytic work, both cation and iodide play roles in phase-transfer and organometallic chemistry, making the salt a staple for tuning conditions and boosting yields in those tough two-phase systems that otherwise stall out.
Synonyms & Product Names
Suppliers often tag this compound as 1-Butyl-1-methylpyrrolidinium iodide or N-Methyl-N-butylpyrrolidinium iodide, and catalogs sometimes carry it under product codes tied to their own inventory systems. Researchers might see abbreviations like BMPyrrI or [BMPy][I] in technical writing or patent disclosures. Anyone hunting for this salt should cross-check these alternate names to avoid confusion, especially as new anion swaps or analogous products show up in the literature.
Safety & Operational Standards
Practical lab safety matters for anything involving organic cations and heavy halides like iodide. Skin and eye contact get flagged as risks, so nitrile gloves and face shielding become standard. Spills need prompt cleanup using absorbents and waste protocols designed for iodine-containing compounds. Waste streams stay segregated from standard aqueous or halogen-free waste for proper handling. Because iodide salts can release small amounts of volatile organoiodine under heating or acid exposure, fume hoods become the obvious choice for bulk reactions or clean-up. There’s a growing push for detailed safety signage and QR-coded safety data sheets, which helps new users catch potential hazards before mishaps.
Application Area
This salt finds a niche in electrochemistry, where it boosts current flow and improves voltage stability in new-generation battery electrolytes—particularly those chasing high energy density and non-flammable properties. Labs active in phase-transfer catalysis and biphasic synthesis gravitate toward this salt for tough organic transformations inside sealed vessels. Materials chemists blend it into ionic polymers or incorporate it into electrochromic devices where cation-anion pairing needs fine-tuning for color change durability. Some groups test it as a template or structure-directing agent in frameworks or nanoparticle synthesis. While not as mainstream as more common ammonium salts, its specialized uses keep it in regular demand across advanced labs.
Research & Development
Academic teams regularly benchmark new ionic liquids against N-Butyl-N-methylpyrrolidinium iodide, using its thermal profile and chemical robustness as a control. Private-sector innovation has lagged some, mostly waiting for costs to drop and commercial demand to rise. Quantum chemists model its charge distribution, hoping to predict new reactivity for catalysis or novel material design. Projects focused on flexible, low-flammability batteries use this salt to push for safer power storage. Each year, new conference presentations highlight modifications of the pyrrolidinium backbone, leading to spin-off products with refined solubility, lower toxicity, or improved conductivity.
Toxicity Research
To date, published toxicity profiles show this salt carries a moderate risk, similar to other small organic iodides. Acute exposure studies—usually using cell cultures or small invertebrate models—flag mild cytotoxicity at higher concentrations, with iodide anion contributing to the impact more than the pyrrolidinium core. Chronic exposure data remain rare, though most responsible handling measures keep real-world risk under control. Environmental groups raise concerns about persistent halides in water systems, suggesting tighter waste controls as volumes scale up. Product safety sheets urge strict adherence to disposal laws for iodine and quaternary ammonium salts to limit long-term ecological effects.
Future Prospects
Looking ahead, the compound’s future in battery and device development looks promising, especially as industries push for safer, non-volatile electrolytes in compact form factors. Researchers project expanded use in organic synthesis and catalysis, largely driven by new green chemistry standards and a search for alternatives to less stable ammonium-based salts. Coatings and specialty plastics might see it emerge as a charge carrier or static dissipative additive. Regulatory scrutiny will increase, so manufacturers who champion green sourcing and environmentally safe disposal methods should lead the pack in adoption. With the tech world scrambling for better energy storage and transport, research into this compound’s variants and analogs promises to deliver even more options in the coming years.
Quiet Hero in Energy Research
N-Butyl-N-Methylpyrrolidinium Iodide isn’t something you chat about over coffee. In labs, though, its place makes sense. Over time, I’ve watched research shift sharply toward cleaner, smarter batteries and new approaches to solar energy. This compound, often called an ionic liquid salt, shows up often in these advanced energy projects. The reason for this choice lies in what it brings to the table: stability, the ability to dissolve things well, and support for chemical reactions that traditional solvents can’t manage.
Electrolytes With a Twist
Most of us take batteries for granted. Inside, the electrolyte keeps power flowing. N-Butyl-N-Methylpyrrolidinium Iodide often shows up in the search for better, longer-lasting lithium batteries and dye-sensitized solar cells. In my experience, the real advantage comes down to thermal stability and non-flammability. Old-school liquid electrolytes often catch fire or degrade under high temperatures. Chemists mix in this pyrrolidinium salt to sidestep those headaches, making batteries last longer and safer—even outside the lab.
Room-Temperature Ionic Liquids Aren't Science Fiction
A few years back, ionic liquids belonged to niche experiments. Today, they’re inching toward mainstream status. N-Butyl-N-Methylpyrrolidinium Iodide stands among the building blocks for these designer liquids. Its use stretches to catalysis—speeding up chemical processes in everything from fuel cells to organic synthesis. Even academic journals highlight how it allows for more efficient electron transfer, bringing down waste and upscaling performance. Adding this compound helps labs avoid volatile organic solvents, which means fewer risks for lab workers and fewer chemical emissions.
Challenges Aren’t Ignored
Anyone curious about science knows that new materials bring baggage. Cost and sourcing pop up quickly—N-Butyl-N-Methylpyrrolidinium Iodide isn’t cheap to produce at scale. Safety also matters. Although ionic liquids score better for fire safety, some researchers raise questions around toxicity and disposal. It's not enough to replace flammable liquids; the full life cycle after use needs more attention. Policies that encourage recycling ionic liquids and green manufacturing methods can tackle these issues before they spiral.
What Comes Next
Only a handful of companies and universities invest heavily in these salts, but the payoff runs large. Better batteries power more devices—more safely. Cleaner energy storage solutions shrink pollution for cities. Students enter chemistry classes now with hands-on exposure to new materials because labs take these applications seriously. Supporting the science behind N-Butyl-N-Methylpyrrolidinium Iodide calls for steady funding and honest conversation about benefits and blind spots. As tech moves forward, people inside and outside labs should pay attention to compounds like this—not because they're headline grabbers, but because they quietly keep the wheels turning.
The Substance Behind the Name
N-Butyl-N-Methylpyrrolidinium Iodide might sound like a mouthful, yet its role emerges in fields that demand both reliability and versatility. Talking chemistry, the compound builds from a pyrrolidinium core—a nitrogen-based five-membered ring—which meets a butyl group and a methyl group. This forms the cation. Iodide, on the other hand, serves as the counterion. The chemical formula for this compound is C9H20IN, with a molecular structure that goes beyond abstract theory and shapes practical outcomes in labs around the world.
Breaking Down the Structure
The pyrrolidinium ring here consists of four carbons and one nitrogen, all in a tight five-membered loop. The nitrogen atom doesn’t sit quietly—it picks up two alkyl side chains, one butyl (—C4H9) and one methyl (—CH3). This makes the nitrogen carry a positive charge, which partners up neatly with the heavy iodide anion (I−). The overall result is a quaternary ammonium salt, which doesn’t trend in headlines, but it shows up across ionic liquid research and advanced synthesis work.
Why Chemical Details Matter
Formula sheets make for dry reading, but getting specific—like knowing the exact arrangement of carbons and the presence of iodide—helps break through confusion in the lab. Mistaking a methyl for an ethyl or substituting an iodide with chloride can change solubility, stability, and even whether a reaction works. Anyone who's tried to replicate a published experiment with an ambiguous structure knows the frustration.
Applications and Impact
Synthesizing N-Butyl-N-Methylpyrrolidinium Iodide demands careful selection of starting materials, typically a pyrrolidine, butyl halide, methyl iodide, and strong reaction control to avoid unwanted by-products. Time spent on synthesis means something only if the end-use delivers—this salt regularly pops up in ionic liquid studies and as a phase transfer catalyst. These roles shape battery electrolytes, organic synthesis, and specialty separations where regular salts fall short.
Health, Safety, and Environmental Considerations
Every lab worker has stories about the surprises chemical handling can cause. Iodide salts, including this one, pose concerns around toxicity and environmental persistence. The quaternary ammonium cation also shows little inclination to break down easily in nature. Gloves, fume hoods, and waste segregation aren’t just legal tick-boxes. They keep chemical work contained, reduce unnecessary exposure, and prevent unwelcome environmental contamination. Companies and researchers have begun to confront the health footprint of ionic liquids more directly, developing testing protocols and safer disposal methods.
Building Smarter Chemistry
Institutions push for greener solvents and less persistent waste, so chemists face the task of redesign or mitigation. Seeking alternative ions, optimizing synthetic steps, or switching to more biodegradable counterions tackles issues head-on. Sharing transparent data on toxicity and environmental impact helps foster a culture of responsibility—nothing beats an open discussion about process improvements across the research community. There’s room for balance: pursuing high efficiency while respecting downstream environmental costs.
Conclusion
Chemists value details—the structure and the formula define function and set expectations. N-Butyl-N-Methylpyrrolidinium Iodide illustrates how a well-understood chemical turns into a workhorse in demanding research. Its careful management, from synthesis to disposal, carves out progress in technology while nudging the field toward smarter stewardship of resources.
Understanding the Material
N-Butyl-N-Methylpyrrolidinium Iodide, a mouthful to pronounce, plays an important role in labs working on electrochemical research, organic synthesis, and advanced battery materials. Its value comes from its ability to serve as an ionic liquid or as a component in complex electrolyte systems. With chemicals like this, safety and stability are always top priorities, not only for compliance but also for keeping research and production schedules on track.
Why Good Storage Makes a Difference
Over the years, I’ve seen labs deal with plenty of accidents due to skipping basic storage precautions. Many chemicals break down if left exposed to the wrong environment. In the case of N-Butyl-N-Methylpyrrolidinium Iodide, moisture in the air poses a real threat. The compound draws in water like a sponge, which can impact purity. Impurities, even in small amounts, tend to throw off finely-tuned experiments or processes.
Safe Storage Practices
Researchers should store this compound in tightly sealed containers. Iodide salts stay more stable in low-humidity environments—think desiccators filled with silica gel or similar drying agents, or cabinets with controlled atmospheres. Temperature swings also present a risk. Many labs stick to temperatures between 2°C and 8°C, commonly found in a standard lab refrigerator. These lower temperatures slow down any natural tendency for the compound to break down, degrade, or react with stray atmospheric moisture.
Direct sunlight makes a bad neighbor for most iodide salts. Light speeds up decomposition and encourages side reactions that aren’t welcome. An opaque or amber-colored storage bottle helps block stray UV rays. Even if a bottle gets opened briefly, returning it quickly to its safe environment keeps it fresher longer.
Handling in the Lab
My first job in a research lab taught me the value of setting up the workstation before opening bottles like these. Keeping gloves, goggles, and lab coats between you and the chemical is just smart—iodide salts are generally low-risk but nobody enjoys accidental skin contact or inhalation. Even small spills can create cleanup headaches, especially if the compound scatters over electronic balances or nearby workspaces.
Dust control matters. Weighing out the compound gently and pouring slowly prevents the fine powder from floating into the air. Some technicians use a local fume extraction hood, which quickly removes any airborne dust and helps maintain a clean working environment. Keeping tools dry ensures that no stray moisture ends up contaminating the main stock bottle.
Disposal and Sustainability
Improper disposal causes more harm than many realize. Iodide salts don’t belong in the regular trash or down the drain. Following hazardous waste disposal protocols keeps labs in compliance with environmental regulations and helps avoid costly clean-up. Training new researchers on these rules saves labs both time and money.
Manufacturers and distributors often supply detailed safety data sheets. Taking a few minutes to read and understand them makes a real difference in workflow safety and chemical longevity. Labs that invest in strong safety and handling habits not only avoid accidents—they protect both researchers and research quality.
Understanding the Chemical
N-Butyl-N-Methylpyrrolidinium Iodide doesn't pop up in most home labs. It’s a specialty compound, often reserved for advanced research or battery labs working with ionic liquids. A mouthful to say, this salt draws researchers in because of its interesting role in solvent systems and electrolytes. Part of its appeal is its stability under normal handling, but digging into lab safety data tells a sharper story.
What the Safety Data Sheets Show
I have gone through many chemical datasheets and remember seeing the typical warnings for salts like this. According to the Globally Harmonized System (GHS) and several safety data sheets, the hazards look manageable with proper protection. The experts classify N-Butyl-N-Methylpyrrolidinium Iodide as an irritant to skin and eyes. Inhalation can irritate the respiratory tract. Swallowing can bring on stomach pains or nausea. This isn’t a compound for careless work—spills and splashes need prompt cleanup, always using gloves, goggles and fume hoods.
There aren’t piles of toxicity studies for this compound. One can check similar pyrrolidinium salts, which show low acute oral and dermal toxicity. Still, the long-term effects have not been thoroughly researched, especially regarding sensitive populations or repeated contact.
Environmental Concerns and Disposal
Many labs overlook what happens to small-batch chemicals after experiments end. Pyrrolidinium salts have a habit of lingering, and iodide compounds often carry aquatic toxicity risks. If poured down the drain, traces might disturb water systems, especially when not broken down at treatment facilities. Responsible labs collect and dispose of even tiny leftovers as hazardous chemical waste, keeping local waterways safer.
Lessons from Handling Similar Compounds
In my old lab days, we saw how easy it is to underestimate niche salts like this. Gloves always turned brownish if left on after spills, which told us our protective equipment was working hard. A few colleagues reported mild headaches after long hours working with similar ionic liquids. After some investigation, we found our fume hood wasn’t circulating air well—one fix eased the symptoms. Small oversights like these teach that vigilance pays off, even with compounds that seem tame on paper.
Improving Safety
Sitting around hoping for more studies isn't enough for anyone in charge of a lab. Proper chemical hygiene practices can cut down on risk—even with “low hazard” taglines. Training every student and worker to respect not just the obvious risks but also the unknowns surrounding lesser-known salts matters. Setting up emergency eyewash stations close to where these substances get handled makes a lot of sense too. Small reminders—like labeling all secondary containers and keeping an up-to-date inventory—go a long way in helping everyone work with confidence.
Room for Smarter Regulation
Chemicals such as N-Butyl-N-Methylpyrrolidinium Iodide slip through regulatory cracks sometimes because they aren't mass-produced or sold to the public. But with the growth of green chemistry and specialized batteries, more labs and startups will want to use them. Pushing for better hazard labeling and requiring basic toxicity data before sale wouldn't cost much, yet it would help labs avoid mistakes that only appear obvious after an accident.
Getting Clear on Quality
N-Butyl-N-Methylpyrrolidinium Iodide stands out in research labs and development settings for its role as an ionic liquid and methylpyrrolidinium salt. The expected purity usually hits at least 98%, which sets a high standard for those involved in chemistry and performance testing. Someone working in battery development relies on this kind of purity since a tiny contamination can throw off an entire experiment. Even if a supplier promises over 98% purity, every responsible researcher checks each batch for color, particle content, and any strange odor. Consistency in this area means reliable results further down the line.
Packaging That Fits the Job
This compound doesn’t ship in a one-size-fits-all box. Most companies offer it in several packaging sizes to cater to a wide range of workers. A small lab might pick up just one gram for pilot work or proof-of-concept experiments, while another group scaling up their investigation might need 5, 10, or even 25 grams at once. It’s not rare to see suppliers list options for 100 grams, or even up to half a kilogram, for teams pushing toward manufacturing or commercial prototypes. The flexibility lets researchers control costs and waste; excess unused product can degrade or pick up moisture, especially in humid environments.
Why DOES Purity Matter?
A single percentage point drop in purity means new worries. Unwanted by-products, leftover solvents, or trace metals sneak in at lower purities, quietly affecting how the chemical behaves. In electrochemistry, a cleaner salt helps avoid unwanted side reactions and boosts battery cycle life. Synthetic chemists trust purity when precision matters. Impurities have a habit of throwing off expected outcomes. When accuracy is central to your results, even small mistakes turn into big headaches.
Safe Handling Every Step Along the Way
With solid packaging and careful labeling, the chemical’s safety and reliability improve right out of the box. Glass vials, amber bottles, or plastic screw-cap jars guard against sunlight and moisture, which can damage the salt and lower purity. Tightly sealed caps cut down on air and humidity exposure, while smaller containers give options for quick use. Most of my colleagues prefer single-use vials over bigger jars to dodge cross-contamination and make documentation easier in the lab notebook. Every small choice here adds up.
Access and Accuracy in Sourcing
Trusted catalogs post certificates of analysis, checking purity and reporting the actual numbers found in each batch. Clear batch records keep researchers in the loop about what’s really inside. This isn’t just a box-ticking exercise; transparent sourcing supports lab reproducibility and makes lab audits less stressful. If you’re looking at a new supplier, request detailed documents: a simple label isn’t always enough.
Looking Ahead: What Labs Need
Demand for N-Butyl-N-Methylpyrrolidinium Iodide won’t drop soon. Better, cleaner materials mean better batteries, slicker separations, and more reliable chemical analysis. Suppliers stay competitive by offering high-purity product in manageable sizes, and keeping everything labeled and documented with care. For scientists and engineers everywhere, it’s those small, clear details that make the difference between a successful experiment and a wasted effort.
