Decades ago, researchers saw real promise in ethers as solvents, fuels, and intermediates. Diethylene glycol dimethyl ether, once known primarily by scientists and process engineers, was adopted for its handy liquid state at room temperature and knack for dissolving polar and nonpolar compounds. Its development stemmed from growing industrial demand during the mid-twentieth century, particularly as sectors like pharmaceuticals and electronics searched for more reliable choices than older, more volatile ethers. Over time, improved chemical synthesis and broader commercial interest made DEG DME more accessible, shifting it from a specialty product to a common lab tool and utility solvent.
Diethylene glycol dimethyl ether, also called diglyme, owes its widespread use to a combination of practical features—clear appearance, very mild odor, low viscosity. It fills the solvent role for complex synthetic reactions, especially where both water and oily compounds play a part. Chemists value it for supporting both organic and inorganic transformation routes. I’ve leaned on diglyme in research labs to dissolve everything from sodium borohydride to larger polymers, thanks to its ability to handle tough solubility challenges.
Diglyme melts near -64°C and boils around 162°C, making it robust in reactions that need flexible temperature control. It breaks from most ethers by not forming peroxides quickly, bringing extra peace of mind in multi-week storage. With a moderate polarity, it bridges gaps between water-based and organic-compound solvents. Density sits roughly at 0.95 g/cm³. Flammability keeps it off the list for home-lab experiments without smoke detectors and exhaust fans—vapors can ignite if ignored. Stability with common acids and bases opens doors for synthetic chemists who juggle many reagent types.
Anyone handling diglyme encounters chemicals shipped with detailed labeling. Bottles and drums are marked with CAS number 111-96-6, hazard diamonds, purity markers, and safety statements—no one wants confusion when mixing for a batch reactor or chromatography column. Technical purity grades reach up to 99.5% for critical applications: those working on battery electrolytes or precision pharmaceuticals absolutely need the assurance that contaminants will remain below detection levels. I’ve worked with vendors who batch-test diglyme and deliver certificates of analysis that match strict pharmaceutical or electronic industry standards, so supervision matters.
Producing diglyme starts from ethylene oxide, passed through stages of glycol formation, then methylation. Manufacturers step through purification, dehydration, and fractional distillation—each phase dials up the product quality. Considerable effort goes into keeping chloride and residual water below a few parts per million, since even trace impurities derail certain catalyst systems. Some academic labs took a DIY route, but large-scale, safe production relies on process controls and tough regulatory checks.
Diglyme acts not just as a solvent, but as an active participant in a chunk of organometallic and reduction chemistry. In Grignard reactions, its oxygen atoms coordinate with magnesium and lithium, stabilizing intermediates. It tolerates strong bases like sodium hydride without losing structure, so it keeps mixtures uniform for hours at reaction temperatures. Certain modifications—such as replacing a methyl group at the molecular tail—shift its solubility range or boiling point, offering narrower custom solvents. Across research labs, chemists tinker with diglyme analogues to steer selectivity or extend its life in reuse cycles.
Diglyme goes by several names in catalogs and shipping manifests: Diethylene glycol dimethyl ether, Bis(2-methoxyethyl) ether, Glyme, or 2-Methoxyethoxy) methyl ether. Pick up a bottle from Sigma-Aldrich or Fisher Scientific and you’ll often see CAS 111-96-6 up front, though MSDS paperwork always lists synonyms. Workers sometimes refer to it simply as “diglyme” among colleagues, skipping longer chemical names for clarity and speed during bench work or between production batches. Synonym confusion can crop up, especially when sourcing from overseas distributors with alternate trade identifiers, so always check labeling.
Working with diglyme gets safer with respect for fire risk and toxicity. National agencies rate it as flammable, so storage far from heat sources and in well-ventilated hazard cabinets matters. Long sleeves and gloves aren’t optional, and spill kits stock enough absorbent material for small leaks. Inhalation and skin contact risks hover in the background, and several studies show repeated exposure leads to nervous system symptoms in lab animals. Factories and research sites need local exhaust and scrubber systems to keep airborne concentrations below recommended limits—regulatory fines for non-compliance hit hard. Any time I handled diglyme spills, company protocols called for eyewash stations and rapid reporting, which kept injury risk near zero and set a precedent for junior staff.
Real-world jobs for diglyme cover more ground every year. Lithium battery designs rely on its high dielectric strength and wide liquid range, supporting safer storage and cycling in modern rechargeable power cells. Organic synthesis labs—both industrial and academic—depend on diglyme for challenging nucleophilic substitutions, sodium/benzophenone reductions, and metal catalyst work. I’ve seen pharmaceutical pilots scale up diglyme-based reactions to hundreds of liters, due to low byproduct formation and minimal contamination—no easy feat in crowded facilities where product recalls can break a company’s reputation. Electronics fields employ diglyme as a cleaning solvent for microchips and circuit boards, especially for flux removal after soldering runs.
The pace of R&D in diglyme chemistry tracks with demand for safer, more adaptable solvents. Universities seek eco-friendly modifications, such as green glyme variants or recycling schemes that recapture solvent before atmospheric release. Innovations around continuous reaction systems hinge on tailored solvent mixes—recent articles highlight diglyme’s compatibility with process chromatic purification and catalysis. Patents pile up on new glycol ether derivatives, with multi-lab collaborations pushing into solar cell and electronic ink advancements. My experience in a university-industry partnership involved screening diglyme blends for biodegradable packaging synthesis, which found surprising success versus crude petroleum-based solvents.
Diglyme’s low acute toxicity led to some early underestimation of its health impact, until deeper chronic studies revealed ties between exposure and organ and nervous system stress in animals. Occupational health specialists flagged reproductive toxicity findings and pressed for stricter worker protections. Data from animal studies indicate developmental toxicity at moderate doses—so workplace rules now cap exposure, require air monitoring, and schedule frequent medical checkups for long-term users. I’ve worked where accident records triggered renewed safety training, showing that even seasoned chemists benefit from reminders about the risks—not just to themselves, but to nearby colleagues and trainees.
Looking ahead, the future of diglyme faces two tracks: industrial growth and regulatory scrutiny. Battery tech companies chase higher capacity lithium cells using diglyme and its variants, but governments around the world now look for substitutes with lower environmental persistence. Academic labs test biodegradable ethers with similar properties, hoping they’ll step in where diglyme historically held strong. Chemical producers push for closed-loop manufacturing lines to capture and reuse every drop. If new solvents beat diglyme’s cost-to-benefit ratio without higher risk, industry may transition, but for now, demand for this workhorse solvent shows no signs of slowing. My expectation is tighter regulations will push the field toward safer, greener alternatives—but knowledge gained from decades with diglyme will steer chemists as they make that shift, so lessons learned won’t go to waste.
Diethylene Glycol Dimethyl Ether, more often called diglyme, isn’t a household name. Maybe you catch it in small text on a bottle label. Maybe you don’t see it at all, though it’s crept its way into some important corners of industry. Diglyme is a clear, nearly odorless liquid that acts as a solvent. This just means it helps dissolve other things. In my college labs, it always struck me how much work solvents do behind the scenes, making impossible reactions actually pan out. Diglyme fills that background role reliably.
Diglyme unlocks reactions for chemists. Think pharmaceuticals: folks use it to help build up some of the backbone materials for medicines, including antibiotics. Chemists prize it when they need to work with very strong metals or aggressive reagents that don’t mix well with plain water or alcohol-based solvents. Diglyme’s unusually high boiling point and ability to dissolve a range of materials make it useful for lab reactions that demand flexibility.
Battery makers and electronics manufacturers lean on it, too. Diglyme helps produce components for lithium batteries—the kind we trust to run our smartphones, laptops, and even electric cars. It plays a role in the manufacturing of specialty polymers, giving plastics their precise properties. I spent a summer on a research team where diglyme was handy for making tiny metal nanoparticles used in electronics. Other solvents just wasn’t up to the job—diglyme brought the right stability to get the reaction going.
Printing inks, adhesives, and coatings sometimes include diglyme. Its low viscosity allows for smooth application and even drying in those uses. The solvent enables inkjet and laser printers to churn out crisp images sheet after sheet. It even sneaks its way into certain cleaning solutions for industrial equipment.
Many chemicals perform miraculous stunts in labs and factories, but you never want to forget the flip side. Diglyme, while less threatening than some, can still affect human health. Prolonged or repeated exposure, particularly in enclosed spaces, potentially causes headaches and nausea. Some animal studies linked it to issues with development, flagging a warning for anyone regularly working with the solvent.
I once saw a colleague get a nasty skin rash from careless handling, and those experiences tend to stick. OSHA guidelines cover the basics: gloves, eye protection, and ventilation. If a spill occurs, immediate cleanup keeps trouble away. Facilities storing the solvent invest in special containment to prevent leaks reaching water supplies. Accidents may be rare, but ignoring risk multiplies the chance of regrettable outcomes.
Industry is never content to stand still. There’s a push to swap diglyme for safer solvents when possible, especially in processes where substitution won’t hurt the final product. The European Union has flagged it because of its toxic profile and tightens how it’s managed. Some newer, “greener” solvents are under development, though matching diglyme’s mix of stability and power challenges even inventive chemists.
It falls to companies, labs, and workers to keep demanding safer work environments without losing the progress that chemicals like diglyme once sparked. Following safety rules, keeping up with new research, and investing in alternatives offers the best shot at reducing risk. The tools change, but the priority—protecting people while making what society needs—stays solid.
Diethylene Glycol Dimethyl Ether, often called diglyme, shows up in a lot of chemical labs and workshops. It solves things that regular water simply can’t touch. Its clean smell can lure you into thinking it is harmless, but diglyme holds some real risks for anyone around it. Just a drop on bare skin can pass right through, and over time, that adds up. I’ve seen folks trust their gloves just because they feel thick, but not all gloves keep out diglyme. Exposure can mess with your liver and kidneys, and breathing in even a little will hit your lungs fast.
Diglyme gives almost no warning before a problem starts. It evaporates quietly, filling a small room with invisible vapor. If anyone forgets to check their workspace’s air flow, the fumes sneak up slowly. Government agencies classify it as hazardous, noting how it’s tied to reproductive harm in animal studies. Once I watched someone pour it in the open, thinking the work would only take a minute. By lunchtime, the air felt heavy, and a headache followed quickly. The lesson stuck hard: never let your guard down, even for a quick job.
Wearing the right gear is the simplest line of defense. Not every glove stops diglyme, so always pick nitrile or laminated gloves—latex doesn’t cut it. Lab coats are good, but full coverage makes more sense: tight cuffs, no exposed wrists. Splash goggles protect far better than standard glasses. Respirators with organic vapor cartridges keep your lungs clear if ventilation runs low. Face shields help for big pours when the risk of a splash jumps up.
A hood isn’t just an accessory—it’s essential. In a proper fume hood, vapors don’t settle in your lungs. From my own time in cramped labs, I learned that skipping the hood after a minor spill always led to regrets. Wipe up every drop using material that soaks up solvents, not the regular paper towels. After cleaning, seal the waste. If it sits open, vapors escape back into the air.
Labeling matters more than most people think. Each container showing its full chemical name keeps coworkers clear and avoids mix-ups that can turn dangerous fast. I’ve sidestepped more than one accident thanks to clear markings left by someone with good habits. Diglyme stored near acids brings fire risk—one small mistake and something can go up in flames. Always keep it in closed metal or high-grade plastic containers, far from heat, light, and anything acidic.
The first aid kit should never gather dust in a cabinet. If spills reach skin, rinse with water straight away—waiting gives the solvent more time to soak in. Paint a clear route to the emergency shower. Don’t block it with carts or boxes. I’ve seen seconds wasted in panic, and that’s when real harm sets in.
You can’t cut corners with solvents like diglyme. Regular safety drills sound boring, but facing an emergency without practice gets messy. Reading the safety sheet isn’t exciting, but it’s the difference between a close call and a trip to the hospital. Ask questions if anything confuses you. Trust your gut: if something smells off, stop work and rethink. Any shortcuts with diglyme rarely end well, so stick to the basic rules. They exist for a reason—and they keep everyone coming home safe.
Diethylene glycol dimethyl ether, often running around chemical supply catalogs under the nickname Diglyme, plays a quiet but firm role behind the scenes in countless chemical processes. Now and then, someone just wants the straight answer: the chemical formula comes out as C6H14O3, and the molecular weight adds up neatly to 134.17 g/mol. But this stuff isn’t just a string of numbers or a formula packed into a bottle. Its impact stretches a lot farther.
Back in grad school, keeping track of the right solvent for the reaction meant the difference between a productive Friday and a headache that stuck around all weekend. No one wants to be caught mixing up Diglyme with something like ethylene glycol dimethyl ether—they may only differ in a couple atoms, but that gap shows up big in how reactions behave. The formula C6H14O3 represents a chain of two ethylene glycol units joined by an oxygen with methyl groups at each end. It’s not just trivia for bored chemists. Knowing the weight, that 134.17 grams per mole, gets you the right stoichiometry. Miss by just a few grams in a scale-up, and suddenly the reaction goes off script, costs rise, and safety concerns snowball.
Most chemists bump into Diglyme during reactions that call for something polar but not ready to step in and react with half the periodic table. It pops up when you need a high-boiling, stable solvent with enough ether in its blood to keep alkali metals or Grignard reagents happy. In the world of batteries, diglyme acts as a solvent that stands up to harsh conditions. Anyone working with lithium batteries or certain types of organic synthesis comes face to face with this liquid sooner or later.
That widespread use ranks diglyme high in importance, but it’s a mixed bag. The tricky part starts showing once you’re asked to clean it up. Diethylene glycol ethers have a reputation for sticking around both in the human body and in the environment. I remember a safety officer telling horror stories about what happens after inhaling a bit of vapor for too long—liver and kidney problems, headaches, things you can’t just shake off like a hangover. It’s not paranoia: studies link exposure to real health issues, especially in places without strong regulations.
Fact is, once you know what’s hiding in that bottle—its formula and weight included—it’s easier to treat it with the respect it demands. Working in a tight lab, I learned to keep containers sealed and the fume hood fans always humming. Diglyme wants to evaporate and find its way into your lungs or water stream, so simple tricks like solvent traps, proper gloves, and waste collection matter as much as a PhD-level knowledge of organometallics.
Plenty of chemists have already started switching over to greener alternatives. Where possible, companies choose solvents that break down more easily or don’t stick around in living tissue. Government agencies in Europe now push tighter controls on substances like diglyme, favoring solutions that protect both workers and the planet. Universities work hard to train a new crop of chemists who look past the convenience of using what’s always worked and try out new, safer solvent systems.
Giving someone the chemical formula or the molar mass only scratches the surface. Diethylene glycol dimethyl ether, with its familiar formula C6H14O3 and weight of 134.17 g/mol, stands for a choice about how we do chemistry—whether in a fancy corporate lab or a classroom mixing beakers. Every reaction and every solvent bottle ties back to human experience: from the safety gear we wear to the way we think about the environment we share.
Walk into any lab supply room, and the sight of upright bottles with old warning labels reminds me of how easy it is to let safety slip. Diethylene glycol dimethyl ether, often found in solvents and research, deserves more respect than just space on a shelf. This isn’t just about ticking a regulatory box. The way you store this liquid impacts both people and buildings long after the workday ends.
This ether stands out because it catches fire at a lower temperature than you might expect. It mixes well with water and almost anything else in the solvent world, which fools people into thinking it’s harmless. My experience: the quickest path to an accident starts with thinking something is “probably safe enough.” Vapors from this ether can irritate eyes and breathing passages, but the bigger danger comes from letting it build up in a closed space. That’s where people get sick or worse.
Real stories give stakes to guidelines. Chemical spills stick in my mind — sticky floors, sharp smells, confusion about which extinguishers actually work. It’s easy to forget that some chemicals like this ether don’t just burn, they can make a fire much worse. Once you’ve seen a fire reignite because someone used the wrong cleaning method, you learn to take warnings seriously.
Treat diethylene glycol dimethyl ether like a guest that could cause trouble if ignored. Don’t store it next to acids or bases; reactive neighbors have ended careers and shut down labs. Keep the containers tightly closed. Every time someone leaves a cap askew, vapors fill the air and someone else pays the price.
Find a cool, well-ventilated area away from heat sources. No tanks, no direct sunlight, no radiators lurking nearby. My old workplace kept these liquids in dedicated flame-resistant cabinets marked in big, ugly letters. It wasn’t just about the look — staff always recognized the danger zones. Labeling gives everyone a chance to avoid mistakes, even on a busy day.
Only people with proper training should touch or move these containers. That’s not gatekeeping — that's experience talking. I’ve watched well-meaning staff learn the hard way that personal protective equipment isn’t optional for these sorts of jobs. Gloves that resist solvents, goggles to cover splashes, and lab coats that don’t leave wrists exposed turn close calls into mere lessons.
Too often I see folks tuck hazardous liquids onto whatever open shelf they find. Policies might say “segregate flammables,” but in practice, someone always shortcuts if there’s no regular training or inspections. The best setups post clear rules right at eye level — no more wondering if something counts as flammable or not.
Spill kits belong near storage points, not locked away in a manager’s office. Cleanup grows messier the longer it takes to track down supplies. Fire extinguishers rated for chemical fires make everyone safer, but only if employees know which one works for which substance. Financial investment doesn’t matter if basic drills and reminders go missing.
Responsibility runs deeper than compliance. Storing diethylene glycol dimethyl ether correctly keeps people out of hospitals and buildings intact for another decade. In a world of quick fixes, simple discipline keeps dangerous events rare. Regular training, honest reviews of storage setups, and a culture that rewards smart choices shape whether this chemical helps or harms.
I’ve spent my share of hours in cluttered chemical storerooms and have seen more than one confused look when a solvent like diethylene glycol dimethyl ether, or diglyme, comes up. It seems straightforward—just pour it in some water and see what happens. Only, in practice, the consequences matter a lot, especially for folks who can’t afford to let a reaction get out of control or chemicals form layers like oil and vinegar when you expected a smooth mix.
Diglyme sits in a category of solvents that share similar backbones to better-known glycols. Lab veterans have seen it used because it dissolves both inorganic and organic stuff. In a university setting, I’ve watched diglyme pour straight into water without drama. No swirling clouds, no stubborn layers—just two clear liquids joining forces. The textbooks agree: diglyme mixes completely with water at room temperature.
This miscibility means that if you tip a flask of diglyme into a beaker of water, you won’t see the liquids separate. Water and diglyme link up, molecule to molecule. The oxygen atoms in diglyme’s structure act like little hands, grabbing water molecules through hydrogen bonding. It’s the same trick that lets other glycols like ethylene glycol or dimethyl sulfoxide blend seamlessly with water.
From an experimental point of view, single-phase mixtures cut out surprises. I’ve been stuck before, waiting out stubborn phase separations that just added hours to cleanup and ruined delicate extractions. Mixing diglyme with water creates one phase, so there’s no waste of time fishing out separated layers. Anyone working with reactions that need smooth, even environments—think sodium borohydride reductions or alkali metal reactions—appreciates this property.
There’s another side to consider. What you pour down a drain doesn’t just disappear. Diglyme’s miscibility with water means it can slip through wastewater systems if disposal isn’t controlled. I’ve seen too many local news stories flare up because solvent runoff isn't treated seriously. The compound itself doesn’t break down easily in the environment. This trait places extra responsibility on labs and factories—wastewater containing diglyme demands solid treatment before release. Data from the EPA points out that accidental dumping leads to contamination, and treatment plants don’t pull diglyme out as they do with, say, oils or greases.
For anyone running a lab or a small plant, training people well closes half the gap. Nobody benefits from accidental mixing or careless disposal. Water testing and stricter labeling of solvent waste bins help too. In labs I’ve worked at, switching from diglyme to less persistent, more biodegradable alternatives sometimes paid off, although it takes real planning. Some industries also use closed-loop solvent recovery systems, which can strip out valuable solvents before wastewater even sees the drain. That sort of investment pays dividends in safer water and fewer headaches.
In short, yes, diethylene glycol dimethyl ether and water form a single blend without fuss. Anyone using this solvent owes it to coworkers and their local community to treat that convenience with care and not just tip it down the sink.
| Names | |
| Preferred IUPAC name | 2-methoxyethoxy)ethoxymethane |
| Other names |
Dimethoxyethane Glycol dimethyl ether Monoglyme DME 1,2-Dimethoxyethane |
| Pronunciation | /daɪˈɛθiːliːn ɡlaɪˈkɒl daɪˈmɛθəl ˈiːθər/ |
| Identifiers | |
| CAS Number | 111-96-6 |
| Beilstein Reference | 1180241 |
| ChEBI | CHEBI:31562 |
| ChEMBL | CHEMBL1542 |
| ChemSpider | 7286 |
| DrugBank | DB01941 |
| ECHA InfoCard | 100.009.184 |
| EC Number | 203-977-3 |
| Gmelin Reference | 82227 |
| KEGG | C01549 |
| MeSH | D004010 |
| PubChem CID | 8177 |
| RTECS number | KL5950000 |
| UNII | 3PBT1O8K4W |
| UN number | UN1164 |
| CompTox Dashboard (EPA) | DTXSID1030657 |
| Properties | |
| Chemical formula | C6H14O3 |
| Molar mass | 134.17 g/mol |
| Appearance | Colorless transparent liquid |
| Odor | Sweet |
| Density | 0.944 g/cm³ |
| Solubility in water | Miscible |
| log P | -0.36 |
| Vapor pressure | 0.46 mmHg (20 °C) |
| Acidity (pKa) | ~24.0 |
| Basicity (pKb) | 1.89 |
| Magnetic susceptibility (χ) | -7.84×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.378 |
| Viscosity | 1.70 mPa·s (20°C) |
| Dipole moment | 2.23 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 308.1 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –589.8 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -3585 kJ/mol |
| Pharmacology | |
| ATC code | V07AY33 |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02,GHS07 |
| Signal word | Warning |
| Hazard statements | H226, H302, H319 |
| Precautionary statements | P210, P261, P280, P301+P312, P303+P361+P353, P305+P351+P338, P337+P313, P403+P233, P501 |
| NFPA 704 (fire diamond) | 1-2-0 |
| Flash point | 93 °C |
| Autoignition temperature | 160 °C |
| Explosive limits | Lower: 1.5% Upper: 17.9% |
| Lethal dose or concentration | LD50 (oral, rat): 5,300 mg/kg |
| LD50 (median dose) | LD50 (median dose): 5,185 mg/kg (rat, oral) |
| NIOSH | WIW3048000 |
| REL (Recommended) | 4 mg/L |
| IDLH (Immediate danger) | 1,500 ppm |
| Related compounds | |
| Related compounds |
Diethylene glycol Dimethoxyethane Tetraethylene glycol dimethyl ether Triethylene glycol dimethyl ether Ethylene glycol dimethyl ether |
