Back in the late 1990s, chemists pushed ionic liquids from the laboratory into practical use, chasing solutions to energy problems and greener industrial processes. 1-Ethyl-3-methylimidazolium chloride-ironum, often known among professionals as [EMIM]Cl–FeCln complexes, grew out of that hunger for more stable, less volatile liquid salts. Early researchers realized that pairing organic cations with transition metal anions opened up electrochemical and catalytic applications, especially compared to plain imidazolium salts. By the early 2000s, journals were dotted with experiments testing its solvent and catalyst capabilities. I first ran across it in a research group struggling to recycle scrap electronics and found it revelatory that such a salt could dissolve metals with so little fuss or toxic byproducts.
The compound pairs 1-ethyl-3-methylimidazolium chloride with iron chlorides to create an ionic liquid. This blend brings up a reddish to deep brown tar-like liquid at room temperature, and its ability to transport and coordinate iron ions gives it a special edge in catalysis, batteries, and electrochemical recovery. While some ionic liquids fade from view due to thermal instability, the addition of iron boosts certain oxidative properties, making it a favorite in both academic and pilot plant settings. Most commercial varieties keep water below 1% and maintain a clear analysis of iron content, usually exceeding 95% purity for chemical work.
1-Ethyl-3-methylimidazolium chloride-ironum boasts a melting point below 60°C, viscosity that hovers close to syrup at room temperature, and extreme thermal tolerance up to 200°C before decomposition begins. Compared to classic molecular solvents, it offers negligible vapor pressure—try spilling it in the hood, and you won’t catch that sharp, unpleasant tang in the air. This property makes a difference during scale-up, keeping the lab benches safer. From my own experience, handling its thick, sticky liquid requires care, but its low volatility means researchers spend less time worrying about chronic inhalation issues. Its density ranges from 1.1–1.4 g/cm3, and because its chloride ions sit free for reactions, the compound dissolves metals and organics that refuse contact with water or common organics.
Labeling for this compound follows strict GHS regulations, given the combination of iron and chloride ions. Purity, water content, and iron oxidation state feature on all reputable certificates of analysis, right alongside batch numbers and exact molar ratios. You’ll want to keep the material in amber glass or Teflon-lined containers, as most metals succumb to corrosion in its presence. In real-world labs, packaging tends to come in 100g bottles or 1L jugs, sealed under nitrogen to resist oxidation. Certificates attach hazard codes for potentially corrosive material and indicate it should avoid contact with strong bases or oxidizers.
Prep starts with mixing high-purity 1-ethyl-3-methylimidazolium chloride with iron(III) chloride under a dry, inert atmosphere. Moisture ruins the product by generating hydrochloric acid—and we have enough burns on our hands to prove it. Most procedures adopt Schlenk lines or glove boxes, using a 1:1.5 or even 1:2 molar ratio for better iron content. The mixture slowly warms to around 80°C, forming a homogeneous dark liquid. Any attempt to shortcut this with tap water or ambient air leaves a rust-colored precipitate and stuck reaction glassware. Product isolation skips crystallization; researchers filter quickly under nitrogen to pull off any iron oxychlorides, cool, and then store airtight.
This ionic liquid shines as both a solvent and reactant. It dissolves rare metals, helps catalyze Diels-Alder and alkylation reactions, and even picks up organic sulfides for chemical separations. Certain researchers swap out the methyl or ethyl groups on the imidazolium ring, adjusting viscosity or tweaking redox properties for specific reactions. The iron center dances between Fe2+ and Fe3+, lending strong oxidizing power during organic synthesis. I’ve watched it strip out noble metals from e-waste in less time than traditional acids could, and it helps shuttle electrons in battery prototype cells.
Among the community, 1-Ethyl-3-methylimidazolium chloride-ironum turns up as [EMIM]Cl–FeClx, or “EMIM Fe(III) chloride ionic liquid.” Some vendors label it as “EMIMCl:FeCl3 complex ionic liquid,” while academic literature sticks with longer IUPAC references like “1-ethyl-3-methylimidazolium tetrachloroferrate(III).” No matter the name, its fingerprint—deep brown hue and strong metal affinity—keeps it recognizable.
Work with [EMIM]Cl–FeClx calls for gloves, face shields, and, ideally, a double-layered lab coat. It burns, stains, and, left unchecked, contaminates benchtops. Even the vapor from warm samples causes mild eye irritation. Standard operating procedures include full fume hood operations, spill kits with sodium bicarbonate, and cold storage below 25°C. Emergency protocols treat it similarly to concentrated hydrochloric acid, though chronic toxicity rates trend lower for the ionic pair. Every reputable lab logs usage and waste by mass, keeping staff accountable and accidental releases traceable, as local environmental laws demand.
Industries rely on this type of ionic liquid for electronic recycling, hydrometallurgical extraction, advanced catalysis, and high-performance batteries. Its low volatility and reusability lower hazardous waste output compared to traditional mineral acids. In our battery pilot projects, [EMIM]Cl–FeClx carried iron ions smoothly between electrodes without the breakdown that plagues organic solvents. Chemists leverage its tunable properties for carbon capture and even biomass conversion, tackling waste in real-world feedstocks where purity wavers. As electronic scrap mounts worldwide, this salt steps up to dissolve gold, palladium, silver, and copper while minimizing side contamination.
Recent papers chase automated recovery of rare metals using continuous processes powered by [EMIM]Cl–FeClx. Startups seek to design larger scale reactors and new extraction agents blended with this ionic liquid. Our own work with university labs showed promise in one-step leaching and separation, especially defeating the problems of toxic fume release found in classic processes. Grants target direct lithium recovery from brines, using these salts to strip out valuable ions where conventional technologies simply fail. Everyone in the field keeps an eye on scalability, aiming for cells and reactors that handle metric tons per day.
Toxicological reviews so far point toward moderate risk rather than extreme hazard. Acute skin exposures irritate, but longer-term injury from environmental release seldom turns up under controlled conditions. Oral and inhalation LD50 values trend much higher (less toxic) compared to legacy chlorinated solvents or heavy metal salts. Ecotoxicology studies tag the iron species for aquatic risk, especially towards algae and crustaceans, but nothing compared to lead or mercury salts. Any spill on soil or into waterways requires prompt cleanup; slow breakdown can release soluble iron and persistent organics, so regulatory oversight and environmental monitoring should match those for mineral acids.
Expect the next ten years to bring blends incorporating not just iron, but entire families of transition or rare earth metals. As demand for clean recycling and renewable energy grows, researchers will pursue better selectivity for critical elements at lower energy cost. Battery manufacturers continue to test new ionic liquids for long-lived, high-voltage cells. Advances in computational chemistry and real-world monitoring offer new ways to predict hazards, guiding safer molecule design. Lab and industry need to work shoulder to shoulder, building both smarter protocols and advanced reactors. Smarter standards will focus on both personal health and persistent environmental footprint, as regulators and the public rightfully push for proof of safety and reduced chemical waste.
Chemists and engineers chase better ways to make and recycle materials. 1-Ethyl-3-methylimidazolium chloride-ironum—a kind of ionic liquid—has earned a spot on the lab bench and production floor thanks to its unique combo of stability, conductivity, and dissolving power. Its iron-containing core brings interesting magnetic properties to the mix, and its imidazolium base keeps it liquid under normal pressures and temperatures. This compound has attracted serious attention in sectors hungry for cleaner processes and smarter materials, and the hype lines up with the results.
Metallurgists often lean on ionic liquids like this one to step outside the limits of old-school solvents. 1-Ethyl-3-methylimidazolium chloride-ironum can dissolve metals such as iron, copper, and gold, cutting out toxic acids and keeping the working environment safer. The regular solvents used in these tasks throw up red flags when it comes to worker safety and environmental protection. Switching to this ionic liquid knocks out fumes and waste problems, making it more attractive for urban mining and electronics recycling. Over the past decade, I have seen big electronics recyclers pivot their R&D towards such technologies—to squeeze out value without poisoning the local water table.
Push for greener chemistry often runs into cost, reliability, and contamination worries. Here, this ionic liquid stands out. It remains stable at higher temperatures, shrugs off exposure to air, and doesn’t spread toxic byproducts like some alternatives. Research in peer-reviewed journals, including Green Chemistry and Journal of Industrial & Engineering Chemistry, has shown its reusability rate stays high over multiple cycles. Compared to volatile solvents that break down after one run, this proves itself as a workhorse—good for both the environment and the budget. Multiple chemical manufacturers are already switching or experimenting with these liquids in pilot plants.
Any material able to move ions and electrons reliably opens new doors in energy storage and smart materials. 1-Ethyl-3-methylimidazolium chloride-ironum supports the push for flexible batteries and capacitors, letting designers tune performance by adjusting concentrations and mix-ins. In universities, I’ve worked with colleagues who explored these liquids in prototype supercapacitors. The results deliver high conductivity and stable cycling. Some teams even tie its magnetic traits to improved energy density. As companies race to build more powerful and greener batteries, this ionic liquid keeps showing up in patent filings and pre-commercial hardware.
Despite its promise, this chemical won’t win over every industrial process overnight. Sourcing high-purity raw materials, scaling up from lab batches, and ensuring regulatory compliance call for up-front investment. Researchers and companies need to keep refining synthesis routes—aiming for cheaper and less wasteful protocols. Industry coalitions could help push for broader testing in critical applications, such as battery manufacturing and metal recycling. Getting buy-in from regulators takes credible toxicity and fate data, not just lab wins. Sharing long-term results across academic and commercial groups would speed up safe adoption.
The world needs more tools like 1-ethyl-3-methylimidazolium chloride-ironum—compounds that make advanced materials manufacturing less toxic and more efficient. Based on real-world results and published data, this ionic liquid clears several hurdles that hold back greener technologies.
I’ve mixed enough reagents and cleaned enough glassware to know that not all chemicals hit the danger list like hydrofluoric acid, but you still can’t throw caution to the wind. 1-Ethyl-3-methylimidazolium chloride-ironum, often called an “ionic liquid,” gets plenty of use in research and industry. Folks see it in batteries, catalysis, solvents, and some advanced materials projects. The fact you usually spot it as a stable liquid, not a powder or vapor, tricks some newcomers into thinking it’s less hazardous. That would be a real mistake.
This ionic liquid pairs an organic cation with iron, and that brings a unique set of risks. Organic ions can give off fishy odors and create skin irritation, but the iron content sets off other alarms. Iron in these compounds isn’t like the iron in your skillet or vitamins. It can jump between oxidation states, participate in redox reactions, and potentially seed the formation of harmful byproducts if the conditions are ripe. Some iron salts corrode metal, and even trace water can change how this liquid acts. Labs have reported catching unexpected stains on stainless steel benches, a reminder that even a small spill reaches out far beyond the bottle.
If you work with this ionic liquid and ignore its quirks, you might notice skin irritation or eye discomfort from vapors, especially if you’re running a hot reaction or working in a confined space. There is not much peer-reviewed data on chronic exposure yet, but the best judgment says keep it off your skin and out of your lungs. I’ve seen cases where careless handling left folks with red, itchy hands for days. If it gets in the eyes, that sting carries for hours, so goggles make a lot of sense.
Long-term exposure to some imidazolium compounds can bring risk to aquatic systems, especially if you pour leftovers down the drain. Researchers have flagged certain ionic liquids as “better than volatile organics” for air quality but not always harmless for waterways. Regulators in the EU and US count these as chemicals of concern. In my lab days, we always sealed the waste in proper containers and marked it for hazardous pickup, never the general trash.
Skip gloves and regret it later. Use nitrile gloves, not latex, and switch to fresh pairs if you spill or splash. Wear a lab coat that reaches your wrists, buttoned up, not tossed over your shoulder. Always use splash-proof goggles, especially if you’re weighing it or transferring to another vessel. Work in a fume hood if you’re heating it or suspect any risk of vapor. Good ventilation means less chance of headache, eye burn, or respiratory complaints.
Keep spills under control with paper towels or absorbent pads designed for organic solvents, and never let metal surfaces sit wet for long. If you spill a major amount, inform your safety officer—sometimes they’ll want more thorough decontamination. Ineffective cleanup only multiplies risk for the next person. Anyone handling this for the first time should get a short walk-through with staff who have used it before. Manufacturers publish safety data sheets that cover basic properties and up-to-date handling tips—read them once, keep them on hand.
Sensible chemical practice means thinking one step ahead. Use less when possible, store bottles tight and upright, check expiration dates, and always keep a spill kit close. Science doesn’t reward the bravest chemist, it rewards the smartest—and that means staying a little paranoid about safety routines every day.
Curiosity about 1-Ethyl-3-Methylimidazolium Chloride-Ironum often starts with its name—a mouthful, but packed with meaning. The backbone comes from an imidazolium core. Picture this: a five-membered ring, two of those spots taken up by nitrogen atoms, and the rest by carbon. Toss an ethyl group onto one nitrogen, a methyl group onto the other, and you’re staring at the 1-ethyl-3-methylimidazolium cation. It might look abstract on a page, but in my own work with ionic liquids, I saw chemists rely on this cation again and again for its stability and ability to dissolve strange things other solvents couldn’t touch.
Pair this cation with chloride, a simple Cl-, and you’ve got a salt. Mix in iron, and you’re spinning the dial: iron joins the dance either as Fe(II) or Fe(III), depending on how it’s made, locking into the mixture as a coordinate complex. Sometimes, iron munches on up to four chloride ions to stable itself as FeCl4-. So, in solution, you find these imidazolium cations floating with iron-containing anions, tied together by ionic bonds. The chemical composition shifts based on the precise ratio, but the underlying play remains the same.
This blend does more than look interesting in a flask. Over years of reading and experimenting, I noticed labs scrambling to find solvents that could handle tough jobs: dissolving metals, catalyzing reactions, or moving heat without catching fire. Traditional organic solvents falter here—flammable, toxic, hard to recycle. Imidazolium-based ionic liquids cracked open a new world. They’re practically non-volatile, stubborn against burning, and reusable. Tossing iron chloride into the mix makes things even more capable for high-performance uses, including green chemistry applications.
In research, you keep bumping into stories where scientists swap toxic reagents for ionic liquids like this one to cut environmental impact. The structure of 1-ethyl-3-methylimidazolium chloride-ironum lets it tackle advanced electrochemistry, recycling rare metals, and separating gases most liquids would barely touch. The iron center can shuffle electrons, making these mixtures prized for redox flow batteries and other energy tech.
For all their promise, these chemicals deserve a hard look before rolling them out on a large scale. From handling samples in school labs, I learned that even tiny changes in composition can shift toxicity, reactivity, or environmental persistence. Proper ventilation and gloves aren’t negotiable with ionic liquids, especially those containing metals like iron. Research is catching up, but so far, 1-ethyl-3-methylimidazolium chloride-ironum shows relatively low toxicity, especially compared to older solvents—yet it still needs smart handling and disposal.
The sunniest future for these materials lies in continued peer-reviewed transparency. Studies comparing the structure, reactivity, and safety of various ionic liquids keep everyone honest. Open sharing of data—especially about potential hazards and environmental effects—keeps industry and academic labs on track. As these liquids edge closer to commercial-scale use, researchers must evaluate lifecycle impacts, not just clever chemistry. I’ve seen how unexpected problems pop up once you move from flask to factory, so careful stepwise scale-ups matter.
Anybody who spends time in a lab knows you can’t just swap old chemicals for new ones without doing your homework. By digging into the structure and composition of ionic liquids like this one, scientists fit the right tool to the right job. With rigorous studies, open discussion, and respect for limits, this powerful mix might push forward everything from recycling tech to safer, cleaner chemical production.
Dealing with ionic liquids like 1-ethyl-3-methylimidazolium chloride-ironum asks for more than just tossing a bottle on a shelf. These compounds carry promise in areas from battery technology to advanced catalysis, but they only deliver results if treated with the respect they deserve. In the lab, every chemist sees what happens when someone ignores storage rules: what could have been a clean reaction becomes a puzzle of unexpected colors and failed tests. Moisture, oxygen, and even lingering sunlight have a real knack for pushing these sensitive compounds down paths you don’t want to follow.
Even in a well-run facility, humidity creeps in through the tiniest cracks. This is a big deal for 1-ethyl-3-methylimidazolium chloride-ironum. The chloride piece and the iron content team up to invite water, and that gives the compound new traits you never bargained for. Once, after someone left a cap loose for just an afternoon, the orange tinge in a ionic liquid deepened and its performance tanked during an electrochemistry project. Silica gel packs and sealed glass bottles are a must. Storing under argon or nitrogen, especially for long-term projects, protects that investment in high-purity reagent.
Leaving the bottle in direct sunlight or even beside a warm lamp on the bench risks slow breakdown. Iron species love to play with light and oxygen—rust and discoloration show up fast. I once saw an open vial left near a window go from clear to murky brown by the end of the week. Not good if your grant rides on reproducible results.
Amber glass stoppers or aluminum foil wrap cut down light exposure. Placing containers in a ventilated cabinet, away from sunlight and sudden temperature swings, makes just as much sense as wearing goggles in a lab.
It seems simple, but temperature swings change everything. Ionic liquids often hold up at room temperature, but summer heat waves or a cold draft can swing their stability. Reliable storage means aiming for a steady, cool spot, usually between 15 and 25°C (59–77°F). Freezers get too cold and attract condensation, which just brings us back to that water problem. Regular fridges sometimes carry enough vibration and cycling to knock loose caps and seals. A lockable, insulated cabinet inside a temperature-monitored room works best for rare or pricey samples. I learned this lesson after seeing false starts on a project where the only difference between failure and success was the storage spot.
The urge to reach for whatever empty bottle is nearby leads to big regrets. Iron ions, chloride, and ionic liquids often react with some plastics or metal caps. I once watched a batch of product degrade simply because the inside of a metal lid corroded after a few weeks. Glass bottles with PTFE (Teflon) lined caps do the job safely. Label every container with the open date and make it a habit to check regularly for signs of corrosion or cloudiness.
Storing this ionic liquid comes down to a mindset of respect. Small steps—dry hands, airtight containers, glass instead of questionable plastics—shape the difference between a dead-end and new findings. In research, reliability grows from these habits. Chemists who treat their materials with care can count on stability, safe handling, and real progress. Anyone can buy a bottle, but only careful storage delivers the value inside.
Anyone working in advanced research, battery tech, or cutting-edge catalysis has probably run into a challenge tracking down unique compounds like 1-Ethyl-3-Methylimidazolium Chloride-Ironum. Unlike sodium chloride or sulfuric acid, this isn’t something that sits on a hardware store shelf. Each order can feel like an expedition, especially when you’re on the clock for a laboratory deadline or prototype milestone.
Some specialty chemical distributors handle orders for ionic liquids, including 1-Ethyl-3-Methylimidazolium Chloride-Ironum. I’ve found sourcing such materials through reputable scientific suppliers—like Sigma-Aldrich, Alfa Aesar, or TCI—often gets you the paperwork and product quality you want. They vet inventory batches, track purity, and keep up with regulations that small internet vendors often skip. Ask any lab technician who’s had a batch go off-spec—cut corners there and you risk wrecked experiments and budget headaches.
Direct sales from smaller chemical startups or international traders pop up if you’re hunting for better pricing or bulk quantities. Still, the lack of consistent quality control has burned plenty of buyers. I’ve learned to look for detailed Certificates of Analysis (COA), not just buzzwords or vague assurances about “research grade.”
Most catalogues list this compound in amounts ranging from a few grams up to 500 grams. These sizes fit academic labs and smaller R&D groups. Production-scale facilities or corporate buyers can usually negotiate custom shipments—kilogram drums, sometimes even multi-kilo lots. The jump in scale brings both price breaks and more paperwork. Import clearances and hazardous material transport take time and coordination. Establishing a business relationship with major suppliers helps keep things smooth, as they already have compliance teams in place.
During one procurement push, I tried to save by sourcing a half-kilo drum from an overseas vendor. Delivery stretched six weeks longer than planned, and customs inspectors nearly seized it over confusion with export codes. The cost saved upfront didn't account for project delays or days spent tracking forms. That experience taught me to look past per-gram pricing and focus on reliability and regulatory clarity.
1-Ethyl-3-Methylimidazolium Chloride-Ironum isn’t nearly as widespread as common reagents, so product identity and purity shouldn’t get brushed aside. Based on my interactions with labs and procurement offices, strong supply chain documentation keeps users protected from unknown impurities. Some suppliers will back up their product quality with guarantees and batch-specific analytical data. If a seller can’t show this, or if they duck questions about storage or shelf-life, walk away.
Shipping and storing this class of chemicals requires the right environment. Packaged wrong, moisture can degrade ionic liquids, iron coordination compounds corrode containers, or both. I’ve seen research shipments arrive with sticky, degraded contents after weeks in a hot warehouse. Always review the Material Safety Data Sheet (MSDS) before placing any order, and double-check that your lab’s safety setup covers storage needs for this category of substance.
Regulation around specialty ionic liquids remains in flux, especially cross-border. Some countries tighten rules on organometallics every year. Institutions can ease this by centralizing their chemical purchasing so every order gets a compliance check before money changes hands. From experience, keeping legal counsel or an EH&S officer in the loop avoids costly mistakes and government fines.
Anyone sourcing innovative new chemicals owes it to their teams to balance cost, quality, and compliance. Few things stall research faster than paperwork snags or a tainted batch. Doing it right doesn’t just protect results—it supports safer, smarter science for everyone.
