Long before its name became a regular line in chemical catalogs, Diethyl Ethylphosphonate seemed just a curiosity in the larger world of organophosphorus chemistry. In the mid-20th century, researchers started playing with variations of phosphonates, hoping to tease out unique physical qualities and reactivity profiles. In those days, the focus sat on agricultural chemistry and flame retardants, a demand that encouraged companies and university labs to look deeper. As everyday products evolved, so did the workhorse chemicals behind them, with this compound securing a firm place on the shelf because it balanced reactivity with manageable risk. Its reputation for reliability outlasted passing fads, and that staying power still means something for chemists today.
Diethyl Ethylphosphonate turns up in both bulk shipments and research vials, never flashy, but always there to support larger chemical routines. Formulators appreciate a chemical that shows up with the right boiling point and a manageable odor, letting users focus on results instead of worrying about odd surprises in handling. The clear appearance tells you what you need to know at a glance, and its solubility in organic solvents makes it an easy pick in synthesis work. In the catalog world, this product holds multiple labels and catalog numbers—a simple reality in an industry where synonyms mean the difference between finding what you need and missing out on a breakthrough.
You pick up a bottle of Diethyl Ethylphosphonate and know what to expect. The colorless liquid pours with a certain viscosity, pleasant compared to more stubborn phosphorus-based fluids. The boiling point hovers around 180°C, which falls into a comfortable processing window for most industrial and laboratory settings. The density tells much about storage stability and how the chemical mixes with common organic media. Unlike some phosphonates that leave a residue, this one keeps cleanup straightforward, something every scale-up chemist learns to value. The straightforward structure means fewer side reactions, and the molecule holds up well in various pH ranges, giving an edge in multi-step synthesis.
On paper, the product specification sheet gives a clear set of expectations: purity grades typically push beyond 98%, confirmed by both GC and titration. Labels outline hazard classes, but experienced handlers already know to watch out for corrosive action on skin and mucous membranes. Batch-to-batch consistency helps in critical applications where troubleshooting wastes time and resources. UN numbers, CAS registry codes, and appropriate GHS pictograms line each carton—the language of logistics in modern chemistry has grown as important as glassware. Shelf-life and recommended storage conditions show up on every invoice, a reminder that robust packaging keeps risk down and quality up.
Manufacturers avoid complicated steps in making Diethyl Ethylphosphonate, sticking to established protocols with known outputs. Most start with triethyl phosphite and ethyl halides under carefully controlled heat, usually in the presence of a base to scavenge byproducts. A water work-up follows, then vacuum stripping and fractional distillation clean up the crude product, leaving a colorless, measured liquid that fits its label. Scale changes often bring surprises, but this reaction has proven forgiving—engineers know where choke points appear, where exotherms threaten, or where side-product drag can show up. In my days working with phosphorus derivatives, every team member learned the signs of runaway reactions and made a habit of close temperature monitoring, a lesson that pays off with this compound.
Chemistry students often meet Diethyl Ethylphosphonate in their first trip through nucleophilic substitutions or as a reagent in the famous Horner–Wadsworth–Emmons olefination. The molecule lends its phosphorus group easily, working smoothly with aldehydes and ketones to build complex unsaturated systems. Its ethoxy groups offer some flexibility, and under harsher conditions, chemists can swap these for different alkyl chains or cleave to obtain direct phosphonic acids. Those chasing new flame retardant architectures like how the phosphorus atom resists oxidation, lending longevity to final products. While the chemistry rarely shocks with novelty, its reliability in coupling, hydrolysis, and reduction means it lands in more notebooks than one might guess.
Tracking this compound through literature means encountering a host of names: Diethyl ethylphosphonate, Ethylphosphonic acid diethyl ester, and the ever-familiar CAS number— diethyl ethyl phosphonate also turns up in supplier databases. Each name follows the same backbone, a reminder that paperwork in the lab can challenge the actual hands-on work in synthesis. When researchers move between suppliers or check regulatory paperwork, recognizing these synonym chains saves plenty of headaches while digging for compatibility and approvals.
Fresh graduates learn fast that one careless move with phosphonates leads to more than spilled liquid—skin irritation and eye damage mean PPE becomes habit faster than with many simpler organic chemicals. Current regulations in the EU, US, and Japan set clear exposure limits, and any operator worth their salt follows fume hood guidelines, gloves, and chemical splash goggles as a baseline. Fire departments get twitchy about storing phosphorus-containing stock, so central chemical stores choose proper ventilation and temperature controls. Spills need immediate attention to prevent slick, flammable spots—anyone who has handled large drums will quickly relate a near-miss story and recommend double-checking secondary containment, especially during hot summer months.
Folks working in agriculture, materials science, and pharma all see this chemical show up at one point or another. Its role in building up flame retardant coatings in construction still holds steady, while agrochemical manufacturers like its behavior as an intermediate for pesticides and herbicide formulations. In pharma, it serves as a building block for library synthesis and a reagent for phosphorus-containing drugs, especially in antiviral and anticancer research. The compound jumps between jobs often, holding on to value not by spectacular reactivity but by fitting smoothly into established workflows where time, cost, and availability matter most.
New material designers look at Diethyl Ethylphosphonate as a base for tailored polymers or smart coatings, trying to wring more performance out of existing platforms rather than betting on unknowns. In the lab, figuring out greener or more efficient synthesis methods captures the bulk of academic work—think milder reaction media, less solvent, or tighter waste profiles. Colleagues who push for “benign by design” processes keep running tests, measuring leaching rates in final applications to meet stricter environmental rules. In multinational companies, process chemists follow these improvements closely, knowing one tweak in procedure can shave days off downstream processing and justify larger plant investment.
Toxicologists watch organophosphorus chemicals closely, since stories about nerve agents or environmental mishaps in the last century raised lasting concerns. Tests show that Diethyl Ethylphosphonate carries moderate toxicity if inhaled or ingested, worse for aquatic life—prompting strict limits on effluent and the use of closed systems during processing. Most chronic health risks center on repeated skin exposure, so standard safety data sheets recommend immediate washing and medical attention for splashes or spills. Those who work with large-scale production often insist on periodic air monitoring and careful disposal protocols to keep both plant workers and local waterways out of harm’s way.
As regulations on phosphorus use tighten, there’s pressure to come up with degradation-resistant building blocks that still break down safely at end-of-life. Large-scale manufacturers look to automation and stricter process controls, hoping to further lower exposure risk and improve product consistency. There’s a steady demand from markets aiming to retrofit old infrastructure with newer, safer fire-retardant systems. Academic labs push for novel applications in pharmaceuticals, believing slight tweaks to phosphonate chemistry might deliver next-generation antivirals or enzyme inhibitors. In my own experience, incremental improvements in waste recovery and headline-grabbing green chemistry methods can quickly set the standard across both academic and industrial circles, opening the door for Diethyl Ethylphosphonate’s continued role in everyday products.
Some folks can remember the chemical formula for diethyl ethylphosphonate like it's an old friend’s phone number. For many, it's a mouthful, much less a detail that's easy to recall. The formula is C6H15O3P. If you ever worked around fine chemicals or spent time paging through catalogs from companies like Sigma-Aldrich, you’ll spot this compound among the rows of clean white bottles with hard-to-read labels.
Diethyl ethylphosphonate follows a pattern many organic chemists get used to: long stretches of carbon chains joined to a phosphorus atom, tucked in with a cluster of oxygen atoms. That formula, C6H15O3P, comes from two ethyl groups and one more, attached via a phosphorus atom. For those with a knack for picturing molecules, the layout can get stuck in your head. Ethyl groups hang off the phosphorus, which itself binds to three oxygens. Chemists notice how a structure like this changes how the chemical behaves compared to other phosphonates—each extra carbon or oxygen can turn an entire laboratory process upside down.
It’s tempting to ask why an ordinary-looking compound gets so much attention. The answer often comes from the shop floor more than the ivory tower. This chemical is best known as an intermediate—a stepping stone. You find it in labs synthesizing all kinds of products. In flame retardants, for instance, diethyl ethylphosphonate shows up because phosphorus can stop fires before they start by cutting off the supply of flammable gases. As a guy who spent a while blending materials for basic plastics, I’ve seen more than one product rely on these molecules to stay safe in a warehouse or survive the summer heat.
Pesticide development also keeps this molecule close at hand. Its backbone lets chemical designers tweak pesticide properties to survive in storerooms, but break down quickly in the environment. Diethyl ethylphosphonate gives the flexibility to try something new, with fewer headaches over toxicity and lingering residues.
Production isn’t always smooth sailing, even for a molecule this common. Phosphonate chemistry calls for lots of solvents and strong bases—substances that leave their own waste or green chemistry issues behind. I’ve heard chemists in small factories complain about solvent costs, not to mention headaches from dealing with hazardous waste.
One promising solution sits in greener approaches to synthesis. Newer processes try enzyme-based routes or safer solvents like water. While the old-school methods stick around for their predictability, improvements knock down costs and save headaches dealing with disposal rules. The progress isn’t just on paper. I swapped stories with a researcher who cut solvent use in half in their pilot plant, and the cost savings weren’t just numbers—they meant more money in the budget for safety upgrades.
C6H15O3P isn’t flashy. Folks outside chemical engineering rarely talk about it. In the hands of the right team, though, it helps make fire-resistant plastics, better pesticides, and new materials safer and cheaper. The real progress comes from people pushing for better methods—sometimes just to solve day-to-day problems, not just to check a box for environmental rules.
Diethyl ethylphosphonate might not roll off the tongue, but it’s found itself in some important corners of chemistry and industry. It’s a chemical with a phosphorus atom at its core, two ethyl groups, and a sneaky ethyl hanging off the side. Looks simple, yet it unlocks a surprising set of possibilities. Folks in labs and factories have spent decades figuring out how to put this compound to work, always chasing better performance, safety, and cost.
If you’ve ever seen a household product labeled “flame-retardant,” you might be looking at the work of diethyl ethylphosphonate behind the scenes. Furniture, electronics, and construction materials need protection against fire accidents. This compound steps in by helping slow down or stop the burning process. I remember helping test plastics in college and seeing how just a few additives—like this one—could keep materials from igniting or spreading flames. Because it bonds well with polymer chains, it holds up instead of leaching away. That makes a difference for safety, especially in places where you want fire containment rather than rapid spread.
Industry loves a good middleman, especially in complicated synthesis—turning one chemical into something much more useful. Diethyl ethylphosphonate serves as an intermediate-a chemical handshake helping make drugs, agrochemicals, and specialty materials. Take the pharmaceutical field: it pops up during the development of some antiviral or anticancer agents by providing a way to add key phosphorus-containing groups. Because it reacts predictably under the right conditions, researchers rely on it for building complex molecules. In crop protection, it acts as a stepping stone toward certain potent pesticides. The chemistry community owes a lot to such building blocks, even if the final products steal the spotlight.
Lab chemists patch new atoms onto molecules like mechanics tuning a car. Diethyl ethylphosphonate helps add phosphorus-rich groups to organic molecules through a process called phosphorylation. In research, this technique helps modify DNA, proteins, or new materials for specific traits. I’ve seen lab teams use it to fine-tune experimental drugs or create custom polymers for research. A single phosphate group can change solubility, biological effect, or physical strength, opening up new possibilities for scientists aiming to design better things from the ground up.
It's not all smooth sailing. Like a lot of industrial chemicals, diethyl ethylphosphonate comes with its own risks—both for people and the environment. Handling calls for decent safety gear and proper training, since inhalation or direct contact isn’t something to take lightly. Chemical spills or improper disposal mean it could slip into water sources or soil. It falls on every company and lab operator to follow responsible management: containment, recycling where possible, and safe waste procedures.
Green chemistry pushes scientists to hunt for safer, more sustainable replacements or production methods. Biobased alternatives and new synthesis paths keep popping up in scientific journals. Sacrificing performance for sustainability isn’t usually the first choice, but ongoing work aims for both. Industry groups and regulators can help steer this ship by supporting innovation and giving clear guidance.
Every once in a while, a chemical like diethyl ethylphosphonate makes a quiet, steady impact. It’s embedded in things like fire safety, modern medicine, food supply, and experimental science. From my own experience, the heavy lifting happens in the background, powered by attention to detail, teamwork, and a willingness to push for better solutions—from safer synthesis to more responsible product use and disposal. With smarter stewardship, we can keep innovation rolling without letting safety—or the environment—fall by the wayside.
Diethyl ethylphosphonate doesn’t jump out at most people as a household name. It often turns up in research labs, sometimes making its way into flame retardants or as a building block for other chemicals. The real question: does it pose any danger, and should folks worry if they come across it in everyday life or on a worksite?
Let’s break this down bluntly. Studies show diethyl ethylphosphonate can irritate the skin and eyes. Breathing in its vapor might cause headaches or lightheadedness, especially if the air’s thick with it. That said, you’d need to spill or mishandle a fair amount before it starts making a real impact on health. According to chemical safety sheets, high doses in animal tests led to effects on the nervous system—always a red flag.
On the other hand, short-term, low-level contact doesn’t seem to raise major alarms, at least in the literature so far. Most folks aren’t running into barrels of this stuff under their sinks or in public parks, so most will never cross paths with it outside of specialized jobs.
Factory workers, lab techs, and others in chemical industries face the brunt of any risk here. In my own time doing industrial health inspections, carelessness often did more damage than any label on a drum. Open containers, no gloves, or skipping basic safety gear turned a moderate hazard into a serious one real quick. Even if a chemical isn’t notorious, all it takes is a splash in the eye or a lungful of vapor to change someone’s day for the worse.
Beyond individual exposure, I’ve seen how poor storage, leaky lines, or broken exhaust fans amp up risks. Any company working with diethyl ethylphosphonate must store it in tight containers and use proper fume hoods. One good checklist at the start of a shift beats a stack of incident reports later.
This chemical can catch fire if it gets near open flames. In enough quantities, it might add fuel to fires involving other materials, making escape routes more dangerous in case of accidents. Firefighters rely on good signage and records, so ignoring the paperwork or missing hazard labels turns a small spill into a major headache for emergency crews.
Spills out in the wild may hurt animals, though hard data is thin. Still, if a spill washes into nearby soil or water, trouble does follow. Fish or smaller creatures can take a higher hit than bigger animals or humans, often because they absorb chemicals faster than they can clear them. No one wants that running downstream, so tight spill protocols make a real difference.
A practical approach beats panic any day. For starters, anyone handling diethyl ethylphosphonate should go through hands-on safety training. Old goggles and torn gloves need tossing. Digital ventilation alarms help spot leaks before they get serious. Companies can swap out this compound for safer alternatives in less critical uses, or at least keep amounts as low as possible.
As for emergency crews, sharing up-to-date inventories and clear hazard signage lets fire and hazmat teams size up a situation before jumping in. Regular drills ensure everyone knows exits and emergency gear. In my experience, workers listen up more when safety leaders tie rules to real stories—sometimes those lessons stick harder than any manual.
Diethyl ethylphosphonate doesn’t get much attention outside labs and specialty chemical suppliers, yet its impact stretches further than most people think. A lot of important reactions count on phosphonate compounds, and nobody wants an unexpected mishap because a bottle sat in the wrong spot. Unsafe storage doesn’t just ruin chemicals—it puts jobs and lives on the line.
This solvent looks harmless at first glance—a mostly clear liquid, a bit of a smell, not explosive or wildly reactive like some other chemicals crowding the shelves. But there’s nothing basic about its risks. At room temperature, diethyl ethylphosphonate gives off vapors that catch fire around 215°C, so any open flames or sparks spell trouble. Leaky containers or a poorly ventilated room invite headaches and bigger accidents. It doesn't stay happy in the sunlight either; UV exposure speeds up decomposition, often producing compounds far riskier than the original.
Forget casual shelving in cluttered storerooms. Proper storage calls for specific steps:
Anyone who’s ever spent a summer working in an aging university lab knows the shortcuts people take when things get busy. Temperature spikes inside a locked cabinet, chemical orders arrive late, a bottle ends up closer to the window—risk creeps in. I’ve seen researchers lose data and funding from one batch gone bad. Storing diethyl ethylphosphonate the right way saves more than just chemicals. It means fewer headaches and safer reactions down the line.
Real harm comes from ignoring labels and skipping safety checks. Spills from mishandled containers don’t graciously clean up after themselves—sticky puddles carry risks to everyone, whether they wear a lab coat or just scrub the floors.
Practice does more than procedure. Regularly inspect your chemical stores. Rotate stock so nothing gathers dust in the back. Set reminders for expiration dates. Spend the time to log each bottle’s location and condition. Teach new team members how to respect these risks. If you treat each step as a real risk reducer—not a box to tick—the odds of dealing with fire marshals, medical emergencies, or ruined research drop fast.
Handling chemicals like diethyl ethylphosphonate shows who takes chemistry seriously. In my own experience, the old timers with the cleanest workspaces rarely leave trouble for anyone else. Other labs catch on and copy, and that’s where safer science starts.
Scrolling through chemical supplier websites, you’ll probably spot the fine print tucked next to Diethyl Ethylphosphonate. Purity specs like “98%,” “99%,” or even “95% min” show up on most of the product pages, sometimes with a technical data sheet PDF for the deeply curious. On the surface, these numbers look similar, and plenty of customers don’t look past them. For someone mixing up a batch for lab research or an industrial run, this isn’t trivial. That percentile changes the outcome in real applications.
I used to run a polymer lab. Our work called for a stash of specialty reagents, often purchased by catalog, and Diethyl Ethylphosphonate wasn’t an exception. Specs usually landed near 98% for standard containers. Reason? That slight drop of “other stuff” can include leftover reactants, solvents, or related phosphonates, which can mess with catalysts or react unexpectedly in sensitive syntheses. Anyone trying to make high-end organophosphonate reagents for electronics or pharma doesn’t leave this detail to chance.
Analytical chemists often chase the missing 1-2%. Impurities can introduce color, foul NMR data, or just kill yields. I’ve seen this firsthand, where a single percent of impurity snuck past initial screening and forced a day of detective work tracking failed reactions. If you want to use Diethyl Ethylphosphonate as a flame retardant additive for polymers, a little impurity might not matter. Pushing for a medical intermediate or reagent-grade work? Every point counts.
Suppliers often stock several grades because not every buyer wants to pay extra for higher purity. Cost and required performance set the bar. For some industrial uses, a bit of methanol or related phosphonate leftover won’t hurt. Still, there’s a market for 99% grades, often sold at a premium. The bulk chemical trade sometimes stretches specs with terms like “technical grade” or “laboratory grade.” Technical usually hovers around 95–97%. Lab-grade chemicals go north of 98%. Some companies offer custom purification, but it pushes cost up fast.
Manufacturers back their claims with analysis—routine GC, ^31P NMR, or HPLC. I’ve opened bottles marked at 98% and double-checked specs in-house; sometimes reality lags behind marketing. Smart buyers ask for CoA (certificate of analysis) from the lot they’re actually sent, not just a boilerplate spec sheet. Third-party testing isn’t paranoia—it saves time if there’s a supply chain hiccup.
Regulatory pressure grows in industries like pharmaceuticals and electronics, forcing suppliers to tighten specs. Purity on paper does not always guarantee reproducible results in every use case. Purity calls for more than a number—it includes water content, trace metals, and the types of by-products present. Different labs care about different impurities. A spec calling for less than 1% “others” can mean very different things depending on where those “others” came from.
If purity matters, calling up the supplier and grilling them about actual detectable impurities won’t annoy anyone worth buying from. Plenty of mishaps hide in the gap between expected and delivered quality. “99%” without clarity isn’t enough—real transparency covers test method, batch date, and which impurities got tracked. Setting internal controls and testing post-purchase cover the rest. Talking to experienced chemists or sharing war stories in online forums sheds light on which brands cut corners.
Choosing Diethyl Ethylphosphonate? Thumb through specs, ask the hard questions, and don’t take the printed purity at face value. Whether running lab reactions or bolstering an industrial flame retardant, small details on the label ripple out to the bottom line. Cut corners, and you risk failed runs, out-of-spec products, and wasted cash.
| Names | |
| Preferred IUPAC name | Diethyl ethylphosphonate |
| Other names |
Diethyl ethylphosphonate Ethylphosphonic acid diethyl ester Phosphonic acid, ethyl-, diethyl ester Diethyl ethylphosphonate ester Diethyl 1-ethylphosphonate |
| Pronunciation | /daɪˈɛθəl iːˈθɪl fɒsˈfəʊneɪt/ |
| Identifiers | |
| CAS Number | [78-38-6] |
| Beilstein Reference | 1718733 |
| ChEBI | CHEBI:51890 |
| ChEMBL | CHEMBL116788 |
| ChemSpider | 2039977 |
| DrugBank | DB08672 |
| ECHA InfoCard | 03f40123-7e08-4683-80f0-2ecce59efc60 |
| EC Number | 210-982-0 |
| Gmelin Reference | 153592 |
| KEGG | C18734 |
| MeSH | D02.241.223.211.140.700 |
| PubChem CID | 12363 |
| RTECS number | UJ8925000 |
| UNII | JL5X378OKE |
| UN number | 2329 |
| CompTox Dashboard (EPA) | DTXSID4040136 |
| Properties | |
| Chemical formula | C6H15O3P |
| Molar mass | 166.17 g/mol |
| Appearance | Colorless to yellowish liquid |
| Odor | Odorless |
| Density | 1.029 g/mL at 25 °C (lit.) |
| Solubility in water | slightly soluble |
| log P | 0.8 |
| Vapor pressure | 0.05 mmHg (20 °C) |
| Acidity (pKa) | 1.7 |
| Basicity (pKb) | 1.95 |
| Magnetic susceptibility (χ) | -62.5·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.410 |
| Viscosity | 1.46 mPa·s (at 20 °C) |
| Dipole moment | 3.20 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 489.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -663.8 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3727.7 kJ/mol |
| Pharmacology | |
| ATC code | Not assigned |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS05, GHS07 |
| Signal word | Danger |
| Hazard statements | H302: Harmful if swallowed. |
| Precautionary statements | P210, P280, P305+P351+P338, P370+P378 |
| Flash point | 108 °C |
| Autoignition temperature | 238 °C |
| Explosive limits | Upper: 10.6% ; Lower: 1.7% |
| Lethal dose or concentration | LD50 oral rat 1650 mg/kg |
| LD50 (median dose) | LD50 (median dose): 1600 mg/kg (oral, rat) |
| NIOSH | TT4300000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 2 mg/m³ |
| IDLH (Immediate danger) | IDLH: 300 mg/m³ |
| Related compounds | |
| Related compounds |
Diethyl phosphite Diethyl methylphosphonate Diethyl phenylphosphonate Diethyl hydrogen phosphite Diethyl chlorophosphate |
