1,2-Ethanedithiol: An In-Depth Commentary
Historical Development
Chemists in the early twentieth century began exploring new thiol compounds as tools for organic synthesis. Among those, 1,2-ethanedithiol started gaining attention for its ability to introduce sulfur atoms efficiently into complex molecules. Back then, crude methods reigned; researchers often worked with less-pure starting materials and learned from the powerful odors and reactive nature of compounds like this one. Over decades, techniques matured. Synthesis and purification processes improved, and a more complete understanding of thiol chemistry emerged. This compound, with its twin –SH groups on a two-carbon backbone, became a staple of synthetic toolkits, especially as researchers dove deeper into heterocyclic chemistry and metal-thiol interactions. The historical trajectory of 1,2-ethanedithiol showcases the broader story of progress in organosulfur chemistry and illustrates how persistence and incremental improvement lay the foundation for turning foul-smelling curiosities into practical assets.
Product Overview
1,2-Ethanedithiol, also known as EDT or ethylene dithiol, often appears as a clear, sometimes slightly yellow liquid. It smells strong – in the chemical world, this gets detected at parts per billion. This material contains two thiol groups, which hand it special abilities for binding to metals, cyclization reactions, and protection of carbonyl groups. The role it plays stretches beyond the lab bench: industries use it in making pharmaceuticals, polymer crosslinkers, and even as a reagent for flavors and fragrances despite its own pungent scent. Purchasers tend to seek this chemical at high purities to avoid interference in research or manufacturing processes. Labs and plants that handle EDT keep it on hand for both classic reactions and new explorations, reminding us that time-tested compounds rarely sit unused.
Physical & Chemical Properties
A physical description of 1,2-ethanedithiol sometimes sounds like a warning sign: it’s a volatile, colorless-to-yellowish liquid, with a boiling point around 146 °C and a melting point just below freezing. It dissolves readily in organic solvents like ether and alcohol, less so in water. Its most memorable physical trait remains its odor, which is powerful and sharp, echoing other thiols. Chemically, it acts as a bifunctional thiol, gives strong nucleophilic reactions, and quickly forms chelating complexes with transition metals. Reactivity comes easy; those two sulfur atoms don’t hide, so care in storage and handling matters. Compared to other thiols, EDT needs airtight, well-sealed containers to keep the fumes under control and contamination low.
Technical Specifications & Labeling
Manufacturers ship 1,2-ethanedithiol in tightly capped bottles, often with clear hazard labels and safety warnings. Purity levels commonly reach 98% or more after distillation and purification. Chemical suppliers typically indicate details like molecular weight (94.19 g/mol), CAS number (540-63-6), structural formula (HSCH2CH2SH), and flash point (53 °C, closed cup). Proper labeling reduces risks, with pictograms showing flammability, acute oral toxicity, and environmental hazards. Regulations enforce clarity here; ambiguous labeling doesn’t cut it with regulators or experienced chemists. These technical details help users manage risk, comply with safety protocols, and plan proper storage or shipment.
Preparation Method
Producers often synthesize 1,2-ethanedithiol through the reaction of ethylene dibromide with sodium hydrosulfide and sodium hydroxide in aqueous ethanol. This classic approach dates back decades and brings a reliable yield of the desired dithiol. The process involves careful separation, as the product readily forms azeotropes and mixes with water or alcohol. Distillation under reduced pressure helps pull pure EDT from the reaction soup, while minimizing loss through volatilization. The process also generates significant waste containing sulfur and halide byproducts, which prompts continual effort to streamline workups, recycle reagents, and minimize environmental impact.
Chemical Reactions & Modifications
Chemists use 1,2-ethanedithiol as both a nucleophile and a chelator in various syntheses. It forms stable five-membered rings with carbonyl compounds, making it a go-to for protecting ketones and aldehydes. In the presence of acid catalysts, it cyclizes quickly to yield dithiolanes, which shield sensitive carbonyl groups during multistep synthesis. The compound’s twin –SH groups enable chelation of soft metals such as mercury, lead, or silver, and researchers use EDT to precipitate, sequester, or detect such metal ions. Alcohols and ethers extract it efficiently, and excess can be deodorized with bleach or hydrogen peroxide if any spills occur. The chemical’s versatility shines in organic transformations like reductive cleavage or selective protection/deprotection steps, where selectivity matters most.
Synonyms & Product Names
Across catalogs and technical documents, 1,2-ethanedithiol goes by several names: EDT, ethylene dithiol, ethane-1,2-dithiol, and simply dithioethylene. CAS number 540-63-6 ties these references together for chemists and industry, sidestepping language barriers or branding quirks. Bulk suppliers sometimes use older names like ethylenedimercaptan, so experience teaches vigilance in double-checking chemical identity before running an experiment or scaling up production. These synonyms reflect a chemical’s long presence in labs and on shop shelves, tracing through decades of evolving nomenclature and company records.
Safety & Operational Standards
Handling 1,2-ethanedithiol means thinking about both acute exposure and chronic risks. Strong, unpleasant odors signal leaks quickly, but sniff tests have no place in proper chemical safety. Vapor inhalation can irritate the respiratory tract, and liquid contact can cause skin or eye burns. Workplaces set up local ventilation, fume hoods, and personal protective equipment for everyone nearby. Spills, though rare, need quick containment and neutralization with oxidizing agents. Regulations across Europe and the United States list it as hazardous, so standard operating procedures focus on storage, transport, and disposal rules. Experienced technicians develop habits to minimize contact and keep the material off hands, skin, and surfaces. Training and supervision come with every shipment, not just the nasty-smelling ones.
Application Area
Researchers, chemical engineers, and industrial chemists apply 1,2-ethanedithiol in a range of fields. Synthetic chemistry leans on its cyclization power for protecting reactive sites or for building dithiolane intermediates. Pharmaceuticals see use in the construction of certain active ingredients and as a step in multi-component reactions. Metal industries employ EDT in the detection and removal of mercury or silver, while polymer chemists add it to drive crosslinking or modify surfaces. Flavor and fragrance companies sometimes harness trace-level reactivity, after careful purification, to produce sulfur-containing notes in food aromas. Its blend of nucleophilicity and chelation keeps it in regular rotation not just for planned syntheses, but for troubleshooting, scavenging, or diagnostic purposes. I’ve relied on EDT in the lab for stepwise deprotection and for scavenging trace heavy metals from solution—a testament to the compound’s functionality when other tools falter.
Research & Development
Research teams worldwide continue to probe new reactions with 1,2-ethanedithiol. Recent investigations include catalytic asymmetric synthesis, new ligand frameworks for transition metal complexes, and applications in environmental chemistry for heavy metal sequestration. Advances in process chemistry connect EDT to green chemistry efforts, such as solvent reduction strategies or novel purification techniques. Researchers explore modified dithiol derivatives, hoping to tune selectivity or reactivity. Investment in automated synthesis has also bumped up demand, as precise, high-throughput reactors need predictable, reproducible inputs like highly purified EDT. Ongoing work in academia and industry validates this chemical as more than a stand-in: tweaks to the structure or the reaction conditions open new doors, driving innovation beyond what the original discoverers could imagine.
Toxicity Research
Detailed toxicity studies flag 1,2-ethanedithiol for its acute risks—exposure at high levels causes significant irritation and, over time, could produce more damaging effects on the liver or central nervous system. Rodent research shows moderate oral toxicity, though the sense of smell makes large-scale human exposure rare. Environmental scientists track its behavior in soil and water, noting its rapid breakdown under oxidative conditions. Chronic toxicity figures less in practical lab settings thanks to strong odors acting as an inadvertent safeguard. Research continues to monitor downstream metabolites, making sure industrial disposal doesn’t seed unintended environmental problems. Most laboratories hedge against risk with secondary containment and high ventilation, but ongoing publication of exposure data helps improve standards year by year.
Future Prospects
Future use of 1,2-ethanedithiol will likely hinge on the growing push for sustainability, reducing waste, and developing safer, more efficient syntheses. Researchers see promise in biotech applications, such as targeted metal chelation or probes for diagnostic imaging, thanks to its bifunctional nature. There’s interest in custom derivatives with less odor or higher selectivity, and machine learning drives discovery of even more efficient reaction partners. As regulations around hazardous chemicals toughen, manufacturers and academics alike need to develop cleaner handling and smarter waste management strategies. As knowledge grows, so does our chance to minimize harm and push the boundaries of synthetic chemistry and industrial technology.
A Sharp Scent With Real-World Uses
Walk past a chemical lab or step into the world of flavor chemistry, and 1,2-ethanedithiol hits the nose hard. Its smell—something between raw onions and burnt rubber—forces a reaction. I’ve handled it before in a research lab. One day the bottle slipped a bit. The stink clung to my hands for hours, beating even the most persistent hand soap. But this foul odor hides a surprising amount of value.
Flavor Chemistry and “Natural” Flavors
Packaged foods get their tastes not from farm-fresh ingredients, but from tiny molecules like 1,2-ethanedithiol. Natural onion or truffle doesn’t scale in a factory, so flavor chemists turn to this compound for its sharp, true-to-life bite. Even people who never enter a lab taste its signature every time they open a bag of chips or a can of soup with “natural flavors.” Sometimes manufacturers use only the tiniest trace—one part per billion changes the whole flavor profile. At that amount, you couldn’t see it or smell it alone, but it is there, shifting from hideous to delicious when blended right.
Heavyweights in the Petrochemical Industry
My uncle works in oil refining, and he long complained about leaks and accidents. To his relief, chemical markers make things safer. 1,2-Ethanedithiol does the job. Pipelines for natural gas or propane stay safer because this chemical gives gas a pungent trace. If a leak sneaks out, anyone nearby gets a warning whiff—no high-tech sensor needed. Without these markers, gas leaks would catch entire neighborhoods off guard.
Fuel Chemistry and Metalwork
Engines don’t run purely on gasoline; some rely on additives for performance and safety. Fuel blends use sulfur compounds like ethanedithiol to balance out unwanted reactions. Metalworkers—especially those soldering or working with fine electronics—use special agents called “fluxes” that clean metal and help things stick together. 1,2-Ethanedithiol’s chemical properties allow it to break down oxidized film, so solder joints hold strong. In my first electronics club experience, we learned flux selection mattered as much as steady hands, and the right sulfur-based chemical held together circuits for our school robots.
Making Medicines and New Materials
Drug discovery starts with small building blocks. Ethanedithiol fits into lots of these early-stage lab syntheses, especially where scientists need sulfur-based rings called thiolanes and dithiocarbamates. These rings show up in antiviral drugs, antibiotics, and even potential cancer treatments. Lab groups don’t shout about their sources, but chemical supply records tie many molecules back to this basic sulfur compound.
Toxicity and Safety
This stuff isn’t a toy. Even a drop on the skin causes irritation. Its vapor bulldozes its way through a room. Most people working with it rely on fume hoods, thick gloves, and chemical splash goggles. A splash or a sniff in an open office would clear everyone out and possibly send coworkers to urgent care. Safety training and accident plans help prevent serious problems in both lab and industrial settings.
Looking for Smarter Solutions
Chemists keep looking for compounds that do the same work as 1,2-ethanedithiol but bring less odor and health risk. Smarter containment systems, better ventilation, and sensor-based warnings offer some peace of mind. Some teams now develop new molecules or slow-release capsules, targeting the essential chemical action but trapping the reek. Innovation marches slowly, but the push for greener, safer chemistry benefits everyone—from lab technicians to neighbors near industrial plants.
The Formula at Its Core
1,2-Ethanedithiol carries the formula C2H6S2. Its structure is straightforward: two carbon atoms in a chain, each holding a thiol group (-SH). The full structural formula looks like HS–CH2–CH2–SH. This isn’t just a dry string of letters and numbers. It tells us how this molecule behaves, how it interacts with other chemicals, even how it smells — and, for folks working in labs or industrial plants, that pungent odor is impossible to ignore.
How Structure Informs Function
Ask any chemist about the -SH group, and a look of familiarity shows up. The thiol group brings reactivity. In ethanedithiol, sticking a -SH at both ends makes for a molecule that acts like a claw, ready to “grab” onto certain metals or fill a role as a crosslinker. Anyone who’s tried removing heavy metals from water might use ethanedithiol to bind mercury or cadmium — it’s effective for trapping what we don’t want in our bodies or the environment.
Years ago, I visited a lab experimenting with methods to recover gold from old electronics. Ethanedithiol’s chemical structure, simple as it appears, let them separate the gold out by forming strong bonds. The process turned complex junk into valuable material, thanks to those sulfur atoms. Real-world impact comes from chemistry at this level, not just large technical installations.
Daily Impact and Safety
Not everyone recognizes ethanedithiol’s name, but many have caught a whiff of its scent. The compound smells somewhere between rotten cabbage and something even less pleasant, which means people use it for more than science. Ever heard of gas leak detectors? Some companies blend ethanedithiol into natural gas because its odor is so detectable even at low concentrations. Gas itself is colorless and odorless; this chemical helps save lives by giving an obvious warning if there’s a leak.
Anyone handling ethanedithiol learns pretty quickly about its hazards. Skin contact stings, and inhaling too much makes for a rough day. Material safety training, gloves, and good ventilation all turn from recommendations into non-negotiables. Schools and workplaces push for safety data sheets, regular training drills, and basic respect for what a small amount of chemical can do.
Where To Go From Here
Chemicals like 1,2-ethanedithiol don’t fade out of use. People's dependence on electronics, clean water, and safe workplaces gives this molecule a permanent role. Increased research funding for greener chemistry helps reduce its hazards. Better containment, safer substitutes, and new technologies built on the same principles are moving in the right direction.
Those sulfur atoms tell a story much bigger than their formula. Anyone interested in making chemistry safer and greener can push for better training, smarter regulation, and finding ways to use strong-smelling, potent molecules with greater care. The story of ethanedithiol is about the ways small molecules shape big changes — in labs, industry, and even in the world outside chemistry.
Understanding 1,2-Ethanedithiol in Everyday Terms
Stumbling across a bottle labeled 1,2-ethanedithiol is hard to forget. That strong, almost offensive smell makes you want to close the cap quickly and open a window. Sometimes called EDT, this chemical features two -SH groups, and anyone who’s worked with it can tell you it leaves a lasting impression on your nose, your gloves, and pretty much any surface.
Personal Experience Handling EDT
I spent a year doing organic synthesis projects that called for EDT. In every lab, the rulebook made it clear: suit up, check your glove integrity, and always work in a ventilated fume hood. After a single careless drop on my glove, no amount of soap fully removed the odor. That direct experience taught me to respect EDT and double-check everything twice.
Toxicity Risks You Can’t Ignore
This chemical does far more than assault your sense of smell. EDT falls into the class of substances called thiols. Both animal studies and workplace incidents point to its toxic potential. Direct contact irritates the skin and eyes quickly, even at low doses. Small amounts in the air bring on headaches, dizziness, and sometimes nausea, especially if someone has trouble with strong odors or preexisting sensitivities. Higher concentrations can trigger real damage to the nervous system and liver. Inhaling the vapor over time harms lung tissue, and spills on bare skin burn and blister.
The Centers for Disease Control and Prevention states that inhaling EDT in poorly ventilated rooms may cause symptoms ranging from sore throats to serious respiratory issues. Anyone who’s spent time in a chemistry lab knows the speed at which strong fumes can spread, carrying risk far past the beaker. NIOSH guidelines urge using full-face respirators for high exposures, and they warn about eye and skin absorption. Government safety sheets classify EDT as harmful if swallowed, harmful in contact with skin, and toxic if inhaled in large amounts.
Protecting Yourself in Real Situations
Reducing the dangers means much more than following lab protocols by rote. Glove material matters—nitrile outperforms latex for EDT. Face shields and goggles cut down on splashes. Fume hoods pull away vapors, but regular checks for airflow keep everyone safer. If cleaning up spills, absorbents and neutralizing agents help, but the real skill lies in avoiding accidents in the first place.
Labeling and storage carry their own risks. Accidental mixing with strong acids or oxidizers can cause hazardous reactions or even release toxic gases. Many chemical injuries come not from intentional use, but from small leaks or mislabeled bottles that sit for months before someone notices the smell.
Learning from Laboratory Problems
Many of the worst stories about EDT come from rushing or skipping small steps. The aftermath usually tells a familiar tale: itching hands, headaches, irritated lungs, and a need to check protocols. MIT and OSHA recommend quick action for spills—a full cleanup kit on standby, immediate medical checks for exposure, and never working alone in small spaces with eight-hour projects and tired eyes.
Solutions Instead of Shortcuts
Chemistry teachers and industrial trainers emphasize real-world drills. Knowing the exit routes, practicing spill containment, and reviewing what happens with exposure create habits that protect everyone in the room. Good ventilation, safe storage, and consistent communication build routines that lower the odds of accidental harm. Personal experience shapes these habits the most, but every published guide and regulatory warning sharpen the focus on what not to forget in busy workrooms.
Why 1,2-Ethanedithiol Raises Red Flags
Anyone who’s spent time in a lab will tell you: some chemicals make more of an impression than others. 1,2-Ethanedithiol does just that, thanks to its extremely strong, skunky odor and its reactivity. This isn’t something you want spilling onto your hands or clouding up your workspace. Its straight-to-the-point stench works as a warning, but the real problems run deeper—risk to health, risk to the environment, and risk of fires if storage gets sloppy.
The Risks: More Than Just Smell
This is one of those compounds that immediately reminds you science means business. A few drops splashed or dripped out of a poorly sealed bottle can leave a room unbearable. Inhaling vapors can give you headaches, nausea, or worse, depending on exposure time. Direct skin contact causes irritation, redness, and even blisters if not washed off quickly. Even safety glasses and gloves sometimes don’t seem enough. In my early chemistry days, I learned this the hard way after a careless lab neighbor left a fume hood unsecured. The entire wing stank for days and students scattered to the nearest exits coughing.
Many forget the fire risk. 1,2-Ethanedithiol catches fire easily and produces toxic gases as it burns. In the hands of someone casual about storage, that can mean a dangerous, smoky mess. No one wants to evacuate a building over a small spill gone wrong.
Smart Storage: Keeping Risks Low
Storing this stuff doesn’t take high technology, but it calls for respect and strict habits. Always use tightly sealed glass containers—plastic just doesn’t cut it for the long haul since this liquid can chew through or cause weird leaching. Labels should scream what’s inside and carry hazard icons you can’t miss. Don’t park the container on an open shelf. Set it inside a rated flammable storage cabinet, away from direct sunlight and any heat source. These cabinets shield more than just inventory; they protect people and buildings from sudden accidents.
Temperature swings speed up evaporation and chemical breakdown. Most labs stick with a cool, dry spot at steady room temperature—think 15-25°C. Add a vapor-tight secondary container for insurance. Some organizations store similar compounds under a blanket of nitrogen to cut oxygen contact, shrinking fire risk and slowing decomposition.
Handling: PPE and Good Habits
Long sleeves and chemical-resistant gloves are non-negotiable. Nitrile gloves work for brief exposure, though butyl rubber is a stronger choice. Splash goggles beat regular safety glasses, especially considering how potent these fumes get in a splash. Never open a bottle outside a working fume hood. The airflow pulls dangerous vapors away and keeps the room livable. Even if a bottle looks pristine on the outside, double-check for leaks, crust, or crusty residue around the cap—these signs scream “replace me.”
Always have spill kits ready. Kitty litter or commercial absorbents tackle small leaks quickly. Used absorbents, gloves, and wipes go into a closed, labeled waste container right away—never toss them into general trash. Regular personal hygiene counts almost as much as high-tech tools in preventing health problems. Soap and water go a long way after handling raw chemicals, before you head back to your lunch or drop your gloves for the day.
The Responsible Path Forward
With every potentially toxic chemical, corners cut today become headaches—or emergencies—tomorrow. Training and discipline keep 1,2-Ethanedithiol from causing harm. More than policies on a page, it takes a culture of speaking up, double-checking, and making safety habits as routine as pipetting solutions. Experience says even one person getting complacent can trigger a whole lot of trouble. The best defense is respect for what’s in the bottle and a willingness to treat the warning signs seriously, every time.
1,2-Ethanedithiol: More Than Just a Smelly Chemical
Anyone who’s opened a bottle of 1,2-ethanedithiol remembers its strong, lingering odor. That powerful scent hints at its unique role in a range of activities most folks rarely consider. This chemical stands out not just for its smell, but for its heavy lifting in both labs and industrial sites.
Longtime Ally in Analytical Chemistry
1,2-Ethanedithiol shows up in labs that dig deep into metals. Chemists searching for trace metals use it to create stable complexes that show up clearly in analysis. Take the world of gas chromatography. Here, specialists rely on this compound to “derivatize” or modify other chemicals, helping molecules behave themselves and move through the equipment at a predictable pace. For sulfur research, the sharp nose of 1,2-ethanedithiol makes detection easier, padding the toolkit used in food science, beverage quality control, and environmental monitoring.
Bridging Building Blocks in Synthesis
Organic chemists often look for ways to build molecules by connecting carbon atoms and protecting sensitive parts along the way. 1,2-Ethanedithiol shines as a protective group for certain carbonyl compounds, such as aldehydes and ketones. By temporarily locking these tricky spots in place, researchers can perform complex reactions without everything falling apart. Removing the protection at the end leaves the desired product in one piece, showing the value of strategic thinking and practical tools in chemistry. Famous syntheses published by respected journals like Journal of Organic Chemistry highlight just how popular this approach remains in modern labs.
Meeting Safety Challenges in Industrial Streams
Industry isn’t just about making new compounds—it also means managing nasty byproducts. In the oil and gas world, producers fight with hydrogen sulfide and similar gases. Left unchecked, these cause corrosion, health problems, and damaging emissions. Adding 1,2-ethanedithiol helps neutralize unwanted sulfur, cleaning up fuel streams so equipment runs longer and the air stays cleaner. In the manufacture of high-performance materials, blocking certain reactive sites with this compound controls the outcome of chemical reactions. Experts in polymer production, pharmaceuticals, and specialty flavors draw on this approach to juggle reactivity with precision.
Challenges and Paths Forward
Safety brings every chemist and operator back to basics. 1,2-Ethanedithiol needs careful handling. Its strong odor isn’t just unpleasant—it warns of its toxicity and potential to irritate the lungs and skin. Workers use proper ventilation, gloves, and protective gear to avoid trouble. Recent research published by Chemical Safety Board points to the need for even tighter protocols and new technologies to cut down accidental exposure. Industry leaders and regulators keep searching for safer substitutes where possible, and engineers test new scrubbers and capture systems to further reduce risk. Green chemistry initiatives push for milder, less hazardous alternatives, aiming for both safety and lower environmental footprint. So far, 1,2-ethanedithiol stands firm in its applications due to its effectiveness, but ongoing innovation keeps the door open for better solutions in the years ahead.
| Names | |
| Preferred IUPAC name | ethane-1,2-dithiol |
| Other names |
Ethylene dithiol
Dithioethylene Glycol dithiol |
| Pronunciation | /ˈiːθeɪnˌdaɪˈθaɪɒl/ |
| Identifiers | |
| CAS Number | 540-63-6 |
| Beilstein Reference | 1207557 |
| ChEBI | CHEBI:41860 |
| ChEMBL | CHEMBL16304 |
| ChemSpider | 12171 |
| DrugBank | DB01830 |
| ECHA InfoCard | 100.030.076 |
| EC Number | 211-195-6 |
| Gmelin Reference | 97150 |
| KEGG | C01242 |
| MeSH | D004993 |
| PubChem CID | 7906 |
| RTECS number | KH7520000 |
| UNII | 3B9W6H4E14 |
| UN number | UN3335 |
| CompTox Dashboard (EPA) | DTXSID6020672 |
| Properties | |
| Chemical formula | C2H6S2 |
| Molar mass | 94.20 g/mol |
| Appearance | Colorless to light yellow liquid |
| Odor | unpleasant; skunk-like |
| Density | 1.116 g/mL |
| Solubility in water | Soluble |
| log P | 0.36 |
| Vapor pressure | 0.4 mmHg (20°C) |
| Acidity (pKa) | pKa = 10.6 |
| Basicity (pKb) | 2.06 |
| Magnetic susceptibility (χ) | -65.5 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.570 |
| Viscosity | 2.51 cP (20°C) |
| Dipole moment | 2.02 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 116.1 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -45.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -5049.7 kJ/mol |
| Pharmacology | |
| ATC code | D08AX06 |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS06 |
| Pictograms | GHS06,GHS05 |
| Signal word | Danger |
| Hazard statements | H225, H302, H311, H314, H331, H373, H411 |
| Precautionary statements | P210, P261, P280, P302+P352, P304+P340, P305+P351+P338, P312, P330, P501 |
| NFPA 704 (fire diamond) | 1-2-0 |
| Flash point | 77 °F |
| Autoignition temperature | 220 °C |
| Explosive limits | 3.2–21% |
| Lethal dose or concentration | LD50 oral rat 785 mg/kg |
| LD50 (median dose) | LD50 orally in rat: 261 mg/kg |
| NIOSH | KV3325000 |
| PEL (Permissible) | PEL: 0.5 ppm (2 mg/m³) |
| REL (Recommended) | 10 ppm |
| IDLH (Immediate danger) | IDLH: 5 ppm |
| Related compounds | |
| Related compounds |
Ethanedithiol
1,2-Ethanediol Ethanethiol 1,2-Dichloroethane 1,2-Diaminoethane |
