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Chemistry always marches forward through a mix of curiosity, necessity, and sometimes sheer accident. In the late 20th century, the chemical in question—O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate—found itself born from that kind of environment. It grew out of research into organophosphorus compounds, a class reshaping industrial chemistry during that era. Those decades saw researchers looking for solutions in agriculture, flame retardancy, and synthesis intermediates. Governments and industries sank millions into ramping up yields and improving functional properties, pushing laboratories to try all sorts of modifications on the phosphorus backbone. As new needs showed up—for safety, cost, and performance—this phosphonate surfaced as a result of that trial and error. Even now, people in labs draw on that work from earlier generations when planning new derivatives or applications.
This compound doesn’t make headlines like some of its more notorious phosphorus cousins, but it plays a steady role behind the scenes. Characterized by its trichloroethyl group attached to a dimethyl phosphonate moiety and a hydroxyl functional group, this molecule offers a lot to chemists in need of reactivity and stability. Structurally, what stands out is the pairing of high electron-withdrawing chlorines with a reactive hydroxyl, which leads to certain predictable behaviors in the lab. Its physical state—typically a colorless to pale yellow liquid under normal conditions—makes it manageable, but no less serious when handled without the right respect. The chemical structure brings reactivity toward nucleophiles and allows it to serve as a building block for more specialized compounds. Its labeling includes visible hazard statements, and anyone familiar with phosphorus-based reagents knows to take the warnings seriously.
In my experience, you learn a lot about a chemical not just by reading data sheets but by working with it. O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate has a distinctive, sometimes unpleasant odor and a density that makes it easy to handle with standard liquid transfer equipment. Like many organophosphorus compounds, it resists hydrolysis in neutral conditions, but strong bases or acids can crack it open, usually with a whiff of chlorine vapor. People in the field know that these dense chlorinated liquids require chemical-resistant gloves, fume hoods, and perhaps most importantly, respect for their volatility and toxicity. This is not something you splash around. Its boiling and melting points fall within ranges typical for similar molecules, and solubility skews toward polar organic solvents—less so in water, thanks to the bulky trichloro tail and methyl groups on phosphorus.
Any conversation about phosphonate chemicals runs right up against safety and labeling. This compound’s technical specifications reflect industry efforts to balance reactivity with shelf stability. Storage at room temperature remains common, but folks make sure to keep it away from open flames, incompatible chemicals, and any source of moisture that might set off an unwanted hydrolysis. The labeling leaves no room for doubt: dangers of respiratory irritation, skin burns, and possible longer-term effects from chronic exposure. Globally, companies ship these reagents inside corrosion-resistant drums, with secondary containment, reflecting direct lessons learned from incidents over the past few decades. Regulators have pushed for stricter occupational standards as more workers engage with organophosphorus chemistry, and nobody wants a repeat of older tragedies caused by lax enforcement or sloppy handling.
Many compounds like this one arise out of the drive for efficiency in organic synthesis. Preparation usually starts from trichloroacetaldehyde (chloral), reacting it with dimethyl phosphite under temperature-controlled conditions. Catalysts speed up this reaction and help ensure selectivity toward the desired hydroxyethyl product. Modern chemists tweak traditional protocols, chasing purer batches or higher throughput, but the approach remains grounded in those basic organophosphorus methods. Post-synthesis work allows for derivatizing the core molecule, using it as a launch point for flame retardants, agrochemicals, or pharmaceuticals. With the trichloro group available for substitution and the phosphonate for esterification or further phosphorylation, there’s a solid case for its continued presence in R&D pipelines.
The real value of O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate lies in how easily it participates in follow-up chemistry. The trichloroethyl group brings a lot of possibilities for substitution reactions. Chemists employ nucleophilic displacement and reduction to craft derivatives with unique physical or biological properties. The hydroxyl group can act as a handle for attachment, allowing researchers to tack on bulky groups for specialized applications. If you follow the literature, you notice how researchers use the molecule as an intermediate for more exotic phosphonates or as a phosphorus donor in certain cyclization reactions. This level of versatility keeps it relevant, especially where other reagents fall short due to cost or reactivity issues.
Depending on the context or the regional language, the same chemical might pass under different trade or systematic names. Common synonyms include dimethyl trichloroethanol phosphonate and trichloroethanol dimethyl phosphonate. Academic articles often stick to the IUPAC name, while industrial catalogs may opt for abbreviated forms. Those different names offer a glimpse into the varied environments where the chemical sees use—from fine chemical catalogs to government safety bulletins. Anyone ordering or reading up on the product needs to stay vigilant about variant nomenclature, since mixing up phosphorus reagents can spell disaster.
Workplace safety in chemical industries has never been negotiable, especially around phosphorus-based organics. Folks working with this compound face genuine hazards, so they gear up with goggles, gloves, full-length coverings, and work behind properly tested fume hoods. Emergency showers and eyewash stations need to be operational at all times. Standard operating procedures involve checking for leaks and spills before, during, and after lab work, reflecting hard lessons from the past. Material Safety Data Sheets inform daily decision-making, but nothing beats what experienced workers pass down about double-checking equipment or keeping antidotes close at hand. Chemical industry disasters fade from newspaper headlines, but the shape of safety protocols shows the marks those tragedies left.
Some chemicals get pigeonholed early and never break out of their original niche. This one, though, pops up in multiple industries. R&D groups test it as an intermediate in producing more complex phosphorus compounds. Folks in polymer science chase its potential as a flame retardant, fighting to meet ever-tightening building and textile codes. Others study how its trichloro and phosphonate groups can be modified for agrochemical or pharmaceutical synthesis, hunting for routes to lower yields or novel bioactive molecules. In academic labs, the molecule gets used as a test structure in reaction mechanism studies, since its blend of functional groups makes it a solid stand-in for a wide range of organophosphorus targets. Wherever it lands, the chemical carries a whiff of the old and the new—its core structure unchanged, its uses constantly evolving.
Most advances come out of slow, collaborative effort—grad students running marathon syntheses, postdocs piecing together structure-activity data, industry teams building reactors for scale-up. Modern research dives into tweaking the molecular scaffold for improved performance in fire prevention, targeted drug delivery, and even nerve agent antidotes. Studies map out how modifications at the trichloro or methyl ends affect reactivity, and whether selective dechlorination delivers safer, more environmentally friendly variants. Journals track these shifts, as do funding agencies hungry for discoveries that balance innovation with reduced toxicity and environmental persistence. In university settings, variations of this phosphonate serve as chemical probes, helping scientists decode how phosphorus interacts with biological molecules or environmental samples.
Whenever phosphorus chemistry comes up, so do questions about toxicity and the long-term fate of these compounds. Animal studies and accident reports set the tone early: eye and skin contact lead to rapid irritation and, prolonged, can cause more severe injury. Researchers track how these chemicals break down in living systems and in the environment. While acute exposure risks tend to dominate training and compliance programs, chronic risks from trace contamination or environmental persistence matter just as much. Some countries demand specialized disposal protocols for even small amounts of waste, reflecting worries about byproducts from combustion or degradation. The push toward greener chemistry continues, with researchers screening for metabolic pathways that could lead to safer breakdown products down the line.
People working with O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate recognize that the next decade brings challenges and opportunities. Demand rises for flame retardants but regulations get tougher. Industry races against time to invent safer replacements, but chemical reality forces incremental change over dramatic leaps. Researchers experiment with alternative haloalkyl groups or look for naturally occurring breakdown pathways that may cut down on lingering residues. In the short term, laboratory breakthroughs push the envelope, but industrial uptake only happens where cost, safety, and performance meet. Stories from the early days of phosphorus chemistry echo in every modern safety meeting or patent application: innovation keeps things moving, but wisdom keeps things safe. Chemical history shows that progress means walking a line between risk and reward—a lesson anybody working in this field lives day in and day out.
O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate sounds complex enough to stop most people in their tracks. Beneath the tongue-twister of a name, this phosphorus-containing compound stands out in chemical industries where fire safety and specialized synthesis have real-world consequences. I’ve come across it while working alongside fire safety engineers who stress about halting the spread of flames and research chemists who constantly push for new ways to build molecules without waste or hazards.
I first learned about this chemical in a plastics manufacturing setting. Companies lean on it for its flame-retardant properties. When blended into polyurethane foams or rigid plastics, O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate helps cut down the risk of fire in furniture, building insulation, and textiles. Phosphorus-based flame retardants stand up better than some of the older brominated compounds, which face heavier regulation due to environmental persistence. I’ve seen its impact in product test labs, where even a thin coating on furniture foam means the difference between a manageable smoke event and a full-scale fire.
Europe and North America limit many older flame retardants, but regulatory bodies have studied this chemical’s lower migration risk and lower toxicity, which keeps it in active use. Its chloride atoms and phosphorus backbone work together: once heat hits, the compound reacts to form a protective char layer, slowing down the reach of flames. Anyone who has ever seen foam furniture ignite too easily knows how much peace of mind comes from fire-resistant materials.
Some chemists talk about building molecules the way carpenters talk about crafting tables—both rely on the right starting materials. In specialty fine chemical and pharmaceutical labs, O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate steps in as a building block for organophosphorus compounds, which serve in medicine, crop protection, and advanced material research. It reacts with diverse starting materials and offers up the phosphonate group—a tool used when chemists need a stable, versatile handle to connect things together.
Medicinal chemists keep an eye on this class of compounds because phosphonates help block certain enzymes, making them valuable in antiviral drug development. Agrochemical researchers also test its structures, pushing for safer weed control or pest solutions. The fact that O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate can slide into a wide range of syntheses shows how crucial it is in research circles looking for the next breakthrough.
Though this chemical helps meet essential needs in safety and synthesis, companies and researchers still look for ways to reduce risks. Handling precautions are standard, but ongoing research could lead to alternatives that break down faster in the environment or don’t stack up in living organisms over time. Industry groups, government labs, and advocacy organizations keep data transparent and accessible, helping the public weigh benefits against risks.
In the end, anyone who cares about safe buildings, innovative medicine, or greener chemistry has a real reason to pay attention to compounds like O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate. Scientific communities keep raising the bar by sharing best practices and hunting for replacements that offer the same safety and utility without legacy problems. That’s progress you can see and feel, from safer couches at home to better drugs on the pharmacy shelf.
Chemical stability defines how long a compound keeps its original properties. Take common lab classics like hydrogen peroxide. If left without a dark bottle and a cool spot, it starts breaking down, losing its punch and potentially causing a mess. Such changes don’t just lead to wasted material; the process can be hazardous—pressure build-up, leaks, or even a container pop can risky for anyone nearby.
Real-life consequences teach the lesson: years ago, in a university lab, an improperly sealed bottle of a moisture-sensitive chemical crumbled into a useless clump, and crystals grew on the rim. Cleaning up required not just gloves and mask, but a lesson in what humidity and light can do. This example isn’t rare, and it shows why solid rules matter—even for experienced hands.
Direct sunlight is an enemy for many chemicals. Some, like silver salts, start to degrade or change their chemistry after just a few minutes under a bright lamp. Your kitchen table example would be table salt—it handles light just fine, but medication or peroxide? Those belong in the dark.
Heat plays another massive role. Aspirin, often found in home medicine cabinets, will break down into acetic acid and salicylic acid if stored in a humid or hot bathroom. This doesn’t just create an odd smell—efficacy drops, and safety can’t be counted on. Even with a tight lid, chemicals absorb energy from temperature swings, setting off unwanted changes and reactions.
Water—whether humidity in the air or a drip from a careless rinse—catalyzes trouble for everything from sodium metal to some vitamins or basic powders. Open a bottle of anhydrous copper sulfate in a damp lab, and it turns from crisp blue to muddy within hours. Extra care with desiccators or drying agents isn’t wasted effort.
Labels with both the date received and opened prevent accidental use past the safe window. In my own workspace, a simple log and color-coded labels cut confusion and reduced loss. It may feel overcautious, but seeing batches stay fresh saves headaches and resources.
Even basic containers make a difference. Amber glass blocks light, tightly threaded caps stop air sneaking in, and insulated boxes cushion against temperature jumps. Specialty chemicals deserve special homes—explosives away from oxidizers, acids below the eye line, volatiles in ventilated cabinets. Even a home garage hobbyist can improve safety with a mini-fridge for peroxides and no open flames nearby.
Regulations like OSHA and the European REACH rules highlight why proper storage isn’t just a worry for large labs. Routine inspection, quick cleanup of spills, and ready access to Material Safety Data Sheets (MSDS) help anyone spot problems early and stay out of trouble. Staff training and a clear plan for old chemical disposal contribute to a safe environment, too.
Even small changes—like grouping by hazard class rather than shelf alphabet—boost safety. Once I started separating acids from bases in my own storage, the odd leaks no longer escalated into corrosive drama. Long-term, such simple steps prevent minor mistakes from growing into disasters.
Products with chemical, electrical, or physical risks bring hidden dangers to daily work. I remember working in a warehouse where we shipped containers of solvents; one spill broke out, and poor handling led to a minor injury and a lot of confusion when nobody could find the right gloves or instructions. Incidents like this stay with me, and they show how easily things can go wrong without real, everyday safety practices.
Before picking up any product, read the label and the safety data sheet. Ignoring that simple step often leads to injuries and mistakes. Hazard warnings aren’t for decoration; they tell you how small errors introduce real risks—chemical burns, lung trouble, or worse. Some products release fumes that seem harmless, but over time, they can cause long-term damage. I’ve seen coworkers develop lingering coughs from casual exposure. The health impacts sneak up.
Basic gear makes all the difference. Gloves, safety glasses, and the right kind of mask have saved me more than once from splashes and dust. Cotton work gloves do almost nothing against solvents—get nitrile or neoprene for chemicals. Your eyes need snug goggles, not just reading glasses. I used to dismiss face shields as overkill until I saw chemical splash across a lab partner’s cheek.
Don’t grab any mask off the shelf; check if you need one that filters particles or gases. Dust from a product like cement won’t block toxic fumes from other substances. People cut corners when the gear feels uncomfortable, but you can’t protect your health later if you risk it now.
Keep potentially dangerous products sealed tight and away from sunlight or heat. I kept spare paint thinner near a window once, and it nearly boiled on a hot afternoon. Store products upright, on solid shelves, with clear labels showing contents and hazard information. Never mix leftovers in random bottles, even just for saving space.
Work only in places with plenty of air flow. Paint, glue, and cleaners pump out vapors that pile up fast in a closed garage or shed. Invest in a vent fan or at least prop open windows. My neighbor once ran a gas-powered generator in his basement—he wanted to stay warm during a blackout, but nearly passed out from carbon monoxide. Safe air is non-negotiable.
Spills happen, no matter how careful you feel. Train everyone in the house or shop to know the cleanup kit’s location and how to use it. Neutralizing powders, absorbent pads, and a sturdy broom are must-haves. Never use water on chemical spills unless the label approves; some reactions get violent. Put up a sign or rope off the area until cleanup is complete.
Government agencies like OSHA and the EPA maintain detailed guidance on thousands of products. Their recommendations aren’t just legal boilerplate; they’re built around research into injury data and product behavior. Review official guidelines regularly and share digestible safety tips at team meetings or with family members. Knowledge only helps if everyone feels responsible for acting on it.
Habit beats memory in daily work. Set a routine: gear up every time, check storage weekly, revisit labels before starting, and teach others. The moments when you skip these steps are the moments things go sideways.
Every chemical comes with two essential tags: the molecular formula and the Chemical Abstracts Service (CAS) number. I spent my grad school days working with a lot of substances. People in the lab always reached for the bottle, squinted at the label, and checked two things immediately. The first was a string of letters and numbers, like C6H12O6. That's the molecular formula, telling you what kind of atoms you’re dealing with and how many. The second was a separate number, something like 50-99-7. That’s the CAS number. It's less glamorous, but trust me, it’s just as important.
The molecular formula reads like a short biography. Each capital letter stands for an element: C means carbon, H is hydrogen, O stands for oxygen, and so on. The digits show how many times each element pops up in one molecule. Some formulas turn out simple, like NaCl for table salt. Others stretch for miles, especially when it comes to things like proteins or fossil fuel derivatives.
I used to think the formula told the whole tale. Over time, I learned that it only tells half the story. You see, substances can share a formula and look completely different—sometimes even act in unexpected ways. That’s where the CAS number becomes essential. Every CAS registry number is unique. These digits act almost like a barcode; they cut through the confusion, pinning down exactly which chemical you’re talking about.
Anyone who’s ever tried to order a chemical through a supplier’s site has felt the pain of almost-matches and funky names. A scientist wants to repeat an experiment, check a result, or make a new product. Mixing up a formula or mistyping the name wastes time and sometimes money. More seriously, getting the wrong compound—or even a mixture with impurities—can be dangerous. Things can spiral when safety protocols rely on people knowing exactly what’s in the bottle.
Situations get messy in big industries, too. Take pharmaceuticals: a wrong substance slows approvals, causes recalls, or raises safety flags. Environmental regulators use CAS numbers to list pollutants for clean-up or restriction. I once did water sampling where we had to match suspected chemicals with regulatory blacklists. Without the right ID, the whole task would have become a guessing game with public health on the line.
People sometimes look baffled when asked for the CAS number. Not everyone carries the Merck Index or have access to expensive databases. The free PubChem or ChemSpider databases have saved me and many colleagues countless hours. Plug in the name, structure, or formula, and the right page gives you both the molecular formula and the CAS registry number, alongside safety info and properties.
Education helps, too. Students learning chemistry should get used to more than just drawing structures; identifying and using proper chemical IDs early saves headaches down the line. Employers can set clear policies for handling and ordering only if staff know which numbers to trust.
A single missing digit in a formula, or a typo in a registry number, can gum up an entire process. As someone who’s worked in both research and small industry labs, I’ve seen minor errors turn into big problems. The world relies on precision, not just to save cash or meet a requirement, but to protect people and the environment. That simple pair—the molecular formula and CAS number—brings clarity in a field where tiny mistakes can stack up.
O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate brings a unique toolkit for chemists, especially those working in synthesis and research. Purity doesn't just hold value for regulatory notes on a datasheet—it shapes the way researchers and manufacturers trust their results and predict their yield. From hands-on work in a university lab to scaling up a pilot project, the question often lands on purity. Not every project calls for analytical-grade material, but a consistent purity grade keeps experimental variables minimized. I’ve seen labs unravel weeks of hard work over the unnoticed presence of an impurity.
Differing industries often push suppliers to respond with a range of grades. Pharmaceutical work and fine organic synthesis projects often push for higher grade standards, sometimes over 98%, to avoid side reactions. Lower grades appeal in bulk applications, like flame retardants, where slight impurities offer little concern compared to the cost savings. I remember sourcing for a synthesis project, and a supplier sent over specification sheets for multiple purity levels. This choice let us weigh risk versus cost, fine-tune our protocols, and avoid wasting time chasing purity higher than our process demanded.
Safety teams squirrel away toxicology reports and safety data sheets for good reason. Impurities, even at low percentages, can skew toxicology, introduce dangerous byproducts, or even raise flammability. Anyone who's run a reaction knows the frustration of mysterious byproducts muddying spectra. More than once, I’ve seen unexpected reactivity tied to a trace impurity, slowing progress and forcing expensive clean-up steps.
Material traceability really matters, particularly where strict compliance rules exist. Reputable suppliers provide clear Certificates of Analysis for different purity levels, covering batch-specific data so no one is left guessing. I’ve worked with suppliers who kept meticulous records, helping our lab pass audits and maintain recurring funding. Loose or inconsistent documentation doesn’t just slow down a project. It can introduce enough uncertainty to send a research proposal back to the drawing board.
Granular testing, transparent batch reporting, and unambiguous labeling support confident buying decisions. Quality checks backed by NMR, GC-MS, or HPLC results go much further than a vague assurance—especially if a project’s peer-reviewed outcome depends on clean reagents. From experience, collaboration with suppliers who invite inspection or offer third-party validation makes a difference. It keeps manufacturers, researchers, and investors aligned on expectations.
Market pressure shapes how widely available different purity levels become. Those demanding tighter specs push chemical manufacturers to invest in better purification or deeper analysis, raising industry standards. Larger buyers, like pharma and specialty chemical firms, have already shifted expectations and created a ripple effect upstream. Startups and smaller labs can encourage this trend by making clear demands for documentation, purity, and accountability with each purchase.
Every order sets a new expectation in the supply chain. Individual research groups, procurement officers, and health and safety teams can play a role by refusing to settle for vague paperwork or ambiguous purity grades. Sharing both best and worst supplier experiences in publications, conferences, or industry forums gives others a roadmap for good sourcing. Transparent communication drives the kind of quality improvements in O,O-Dimethyl-(2,2,2-Trichloro-1-Hydroxyethyl)Phosphonate—and countless other compounds—that serve everyone in the long run.
| Names | |
| Preferred IUPAC name | Dimethoxy-(2,2,2-trichloro-1-hydroxyethyl)phosphane |
| Other names |
Fosthietan Dimethyl 2,2,2-trichloro-1-hydroxyethylphosphonate |
| Pronunciation | /ˌdiːˈmɛθ.ɪl ˈtraɪ.klɔːr.oʊ ˈhaɪ.drɒk.siˌɛθ.ɪl fɒsˈfəʊ.neɪt/ |
| Identifiers | |
| CAS Number | 15987-85-8 |
| 3D model (JSmol) | `load =O,P(OC)(OC)(C(O)(Cl)(Cl)Cl)` |
| Beilstein Reference | 2478526 |
| ChEBI | CHEBI:39003 |
| ChEMBL | CHEMBL2106356 |
| ChemSpider | 4205963 |
| DrugBank | DB08693 |
| ECHA InfoCard | 03e2c260-bc51-3df0-a20c-c5dc6c2e3f11 |
| EC Number | 238-118-6 |
| Gmelin Reference | Gm 917588 |
| KEGG | C18473 |
| MeSH | DDT |
| PubChem CID | 27426 |
| RTECS number | TD6125000 |
| UNII | A2J16P45T9 |
| UN number | UN3018 |
| CompTox Dashboard (EPA) | DTXSID8022535 |
| Properties | |
| Chemical formula | C4H8Cl3O4P |
| Molar mass | 249.45 g/mol |
| Appearance | Colorless to pale yellow liquid |
| Odor | Odorless |
| Density | 1.69 g/cm³ |
| Solubility in water | slightly soluble |
| log P | 0.83 |
| Vapor pressure | 0.00016 mmHg at 25°C |
| Acidity (pKa) | 1.62 |
| Basicity (pKb) | 7.48 |
| Magnetic susceptibility (χ) | -49.5e-6 cm³/mol |
| Refractive index (nD) | 1.471 |
| Viscosity | Viscous liquid |
| Dipole moment | 4.98 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 389.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1075.9 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1574.2 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | V03AB26 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes skin irritation. Causes serious eye irritation. May cause respiratory irritation. |
| GHS labelling | GHS02, GHS05, GHS07, GHS08 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H302, H319, H332 |
| Precautionary statements | P261, P264, P271, P272, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P332+P313, P362+P364, P403+P233, P405, P501 |
| NFPA 704 (fire diamond) | 3-1-2-W |
| Flash point | Flash point: 113°C |
| Autoignition temperature | Autoignition temperature: 400 °C (752 °F) |
| Lethal dose or concentration | Lethal dose or concentration: LD50 oral (rat): 3200 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral-rat LD50: 3500 mg/kg |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.1 mg/m3 |
| IDLH (Immediate danger) | IDLH: 100 mg/m³ |
| Related compounds | |
| Related compounds |
Dimethyl methylphosphonate Dimethyl phosphite Trichloroacetaldehyde (Chloral) Diethyl (2,2,2-trichloro-1-hydroxyethyl)phosphonate |
