Sulfuryl Chloride SCl—History, Properties, Uses, Risks, and Scientific Outlook
Historical Development
Sulfuryl chloride, known to chemists as SO2Cl2, has a long timeline that hooks heavily into the growth of industrial chemistry in the nineteenth century. Chemists realized early on that this reactive compound could open new doors in synthetic chemistry and large-scale production strategies. The investigations of sulfur and chlorine compounds started to pick up speed as scientists aimed to underpin modern chemical industries. Throughout the twentieth century, the demand for new synthetic routes, including those for dyes, pharmaceuticals, and pesticides, frequently called for reliable chlorinating agents. Sulfuryl chloride carved itself a firm spot simply because nothing else brought the same blend of reactivity and relative ease of handling. My time in laboratory environments always confirmed what early chemical pioneers saw: the clear value of SO2Cl2 in pushing innovation and meeting practical challenges as industries chased faster and cleaner chemical routes.
Product Overview
At room temperature, sulfuryl chloride lands as a colorless, fuming liquid with an intensely sharp odor. It does not act coy—the pungency and volatility set a clear boundary about safe handling. Across factories and research settings, the focus falls squarely on harnessing its chlorine-donating potential, especially in tasks like converting alcohols to alkyl chlorides and introducing sulfonyl groups. Bulk manufacturers rarely keep it on hand for long—sulfuryl chloride does not store well, and few forget its knack for corroding metal and glass stoppers alike. In chemical warehouses and production facilities, the “handle with respect” rule never loses relevance.
Physical & Chemical Properties
With a molecular formula of SO2Cl2, it weighs in at about 134.97 g/mol. The boiling point sits close to 69°C, while freezing comes at –54°C. The vapor carries a noticeably acrid whiff, and even a small spill makes the eyes sting. Chemically, sulfuryl chloride sits on a razor’s edge—moisture turns it caustic with hydrochloric and sulfuric acids; contact with organic matter or metals can spark fire or hazardous fumes. Every experienced bench chemist knows what a small splash can do to a lab coat or a metallic tool—corrosion spots become hard reminders.
Technical Specifications & Labeling
Standard drums and cylinders show the UN number 1834 and the relevant hazard labels: corrosive, toxic, and environmentally dangerous. Commercial grades demand purity levels above 99%. Impurities, especially water, unleash dangerous decomposition, propelling most suppliers to emphasize airtight, moisture-proof sealing. Manufacturers also include clear usage instructions and emergency guidance. Labels usually cite both CAS number 7791-25-5 and synonyms like sulfuryl dichloride, leaving no room for error. In my work documenting chemical inventories, the regulation-driven clarity around sulfuryl chloride stood in contrast to older, sloppier labeling seen on less hazardous kin.
Preparation Method
Sulfuryl chloride comes from direct chlorination of sulfur dioxide at controlled temperatures around 30–80°C, using activated carbon or camphor as catalysts. The reaction, SO2 + Cl2 → SO2Cl2, rolls out inside specially lined towers with careful control over gas feed. This method keeps the product reasonably pure and scalable, but cutting corners on moisture exclusion leads fast to byproducts and even violent side reactions. From accounts of plant visits and training sessions, one message stands clear—meticulous monitoring is not negotiable to ensure the quality and safety of every batch.
Chemical Reactions & Modifications
In organic labs, sulfuryl chloride’s main currency is its ability to donate both sulfonyl and a pair of chlorine atoms. It reacts with hydrocarbons in presence of light or proper initiators, generating alkyl and aryl chlorides. Alcohols, amines, and phenols all become targets—SO2Cl2 transforms them not only to chlorides but often to sulfonates or other functional groups if conditions swing acidic. Beyond substitutions, sulfuryl chloride helps build sulfonamides and sulfonate esters, mainstays in drugs and advanced materials. In dealing with tough reaction mixtures in grad school, I came to respect SO2Cl2 for its clean conversions—though the need for meticulous ventilation always kept my shoulders tense.
Synonyms & Product Names
Across supplier catalogs, sulfuryl chloride might appear under names like sulfuric dichloride, SO2Dichloride, or even chlorosulfonic oxide. Trade names rarely diverge far—regulatory rules force clarity, given the risks. In many languages and markets, simply spelling out SO2Cl2 sidesteps confusion. Working with international teams, I learned fast that double-checking local nomenclature bridges safety gaps and prevents mix-ups.
Safety & Operational Standards
Personal protection matters above all—no shortcuts get tolerated. Chemical-resistant gloves, eye protection, and face shields stand as minimum requirements. Fume hoods and positive ventilation keep air clear. Storage rules run strict: away from moisture, sealed containers, clear labels, and no proximity to organic matter or reducing agents. Emergency showers and eyewash stations must remain within sprinting distance. Regular training reinforces these habits—not unlike muscle memory from sports. After handling SO2Cl2 during lengthy syntheses, decontaminating glassware felt less like routine and more like an obligation to future safety.
Application Area
Sulfuryl chloride does heavy lifting in agrochemicals and pharmaceuticals, especially as chlorinating agent. Pesticide manufacturing banks on its ability to drive chlorination without byproduct headaches. Pharma companies turn to it for attachment of functional groups that standard chlorine gas can’t manage so cleanly. SO2Cl2-derived intermediates feed into polymer synthesis, dye production, and the surface modification of advanced materials. I’ve worked with coatings engineers speculating on new polymer backbones—their feedback boiled down to reliability, consistent reactivity, and the avoidance of side reactions that plague alternative reagents.
Research & Development
Innovation in chlorination chemistry tracks closely with sulfuryl chloride’s evolution. Researchers keep pressing for methods that minimize waste and eliminate side products, using microreactors and flow chemistry to keep reaction scales safe and manageable. Environmental management pushes greener practices, such as recapture systems for vented byproducts and alternatives that combine efficacy with reduced ecological risk. In literature and presentations, the pivot toward sustainability challenges both suppliers and end users to think beyond classic processes. I’ve seen younger chemists eager to adapt smaller, leaner setups—these bring both cost savings and a sharper safety margin.
Toxicity Research
SO2Cl2 brings real toxicity concerns—breathing the vapor or accidental contact with skin causes severe burns or long-term lung damage. Chronic exposure damages airways and can sensitize workers, making hazardous exposure a genuine occupational risk. Regulatory data underscores strict personal exposure limits, and every reported lab incident prompts renewed safety briefings. Plenty of toxicology studies focus on corrosive effects on mucosa and the cumulative damage to organic tissue. Reviewing case reports and safety data sheets, I feel the weight of chemical stewardship—a few careless minutes can translate into lifelong injury or health risk.
Future Prospects
Research keeps painting new possibilities—modifications of SO2Cl2 for more targeted, selective reagents stand on the horizon. Laboratories experiment with optimizing catalysts and reaction environments to boost precision in industrial scale chlorinations. Robotics and automation offer safer, more controlled exposure for hazardous tasks, which may become standard as technology advances. Environmental concerns drive innovation to cut both emissions and accidental leaks, blending process refinement with engineered controls. In my teaching and consulting, I see young chemists eager to combine tradition and new tools, motivated by sustainability and a fresh commitment to responsible manufacturing.
Sulfuryl Chloride: More Than a Simple Reagent
Walk into any industrial chemistry lab or specialty manufacturing facility, and odds are you’ll spot a few steel drums or specialty bottles marked Sulfuryl Chloride (SO2Cl2). At first glance, it’s just another pungent, colorless liquid with a reputation for being tough to handle. But beneath its sharp smell and fuming character, this chemical carries real weight—mostly because it helps pave the way for making products many people barely think about.
Where the Industry Puts Sulfuryl Chloride to Work
Most folks outside chemistry circles have never heard of Sulfuryl Chloride. In big chemical plants, technicians and scientists turn to it for a few specific reasons. One of its strongest points is its role in making sulfonyl chlorides and sulfonamides, which are building blocks for things like pharmaceuticals, dyes, and certain pesticides. Without this stuff in the production pipeline, companies would struggle to create several medications or vibrant colors in products that line shelves at the local store.
Besides pharmaceutical and dye manufacturing, Sulfuryl Chloride finds its way into the rubber industry. When making synthetic rubbers, it brings the right chlorine atoms into polymer chains—a step that changes how rubber holds up under stress and exposure to different environments. This kind of chlorination makes hoses, seals, and belts more durable, especially when exposed to chemicals or heat.
Another clear use sits in organic chemistry labs, where researchers rely on it to introduce chlorine atoms into all sorts of molecules. Imagine chemists drawing up new ways to make a molecule more effective or less reactive; Sulfuryl Chloride helps pull off these experiments. With its knack for transforming structures, new reactions become possible, and some of those lead to products that eventually make their way into the broader market.
Safety and Environmental Concerns
If someone gets careless with Sulfuryl Chloride, the situation turns dangerous quickly. It reacts with water to create hydrochloric acid and sulfur dioxide, two gases that hurt the lungs and corrode equipment. These risks demand respect and strict training—not just for the sake of the staff, but also for those living near production sites. Proper ventilation, tight handling protocols, and emergency tools like neutralizing agents stand as barriers between routine use and health emergencies.
On the environmental front, even small leaks or spills can cause major headaches. Regulators in the US and Europe watch how companies store and transport this chemical, sometimes forcing them to update their safety guidelines as new research comes in. Engineers and chemists work together to keep emissions as low as possible and develop better containment strategies. These efforts pay off, reducing the chance of accidental releases that could endanger workers or the surrounding community.
Looking Ahead: Solutions for Safer Handling
While Sulfuryl Chloride won’t disappear from production floors any time soon, there’s always room to raise the safety bar. Companies invest in wristband gas sensors, automated valve systems, and employee training built around case studies from real incidents. Some teams also look into alternative reagents—chemicals that deliver similar results with lower environmental costs or less risk to workers.
My own time in a research facility showed how fast things can go south with aggressive chemicals like Sulfuryl Chloride. Respect for its hazards, solid teamwork, and honest communication go a long way in keeping everyone safe, and they set an example worth following across the industry.
Understanding the Risks of Sulfuryl Chloride
Anyone dealing with sulfuryl chloride knows how aggressive this chemical can get. You don’t have to be a chemist to see why treating it like ordinary lab stock is a recipe for trouble. It doesn’t just irritate skin or eyes—it can rip right through organic matter and give off hazardous fumes with just a hint of moisture. Stories about careless handling aren’t scare tactics. I’ve watched colleagues in research environments dodging an emergency after a splash or whiff. Coming away with just a lesson and minor burns counted as lucky.
The Gear that Makes a Difference
Goggles aren't enough. Face shields offer real protection if a flask breaks or a splash jumps out. Butyl rubber gloves shield skin far better than latex. I’ve found lab coats with fitted cuffs keep droplets off my arms, but they need a chemical-resistant apron layered on top for anything beyond measuring a gram. Closed shoes—never sandals or sneakers—complete the picture. Those who’ve walked into an ER with acid burns from splashes landing on feet know why.
Why the Right Space Matters
A strong fume hood stands between you and the fumes sulfuryl chloride gives off. Even a slight reaction with water in air triggers hydrochloric acid and sulfur dioxide gas. Breathing those does more than sting. Investing in good ventilation beats counting on open windows. Doors should stay closed to keep fumes from drifting. I’ve seen labs with simple warning signs outside fume hood zones—a reminder not to wander in with your sandwich.
Storage Routines that Prevent Accidents
Sulfuryl chloride finds ways to break containers not made for it. Glass with screw caps barely lasts a season before cracks show up from the inside. High-grade polyethylene bottles, stored tight with no chance for leaks, save time and money. I always add a label with a warning about water and strong bases—folks need to think twice before stacking it near a sink. A spill inside a shared fridge creates chaos. Dedicated cabinets for oxidizers with spill trays underneath keep small incidents from turning into major events.
Mixing and Diluting—Where Mistakes Happen
A lot of trouble comes from rushing. I set up all materials in advance, double-check weights, and keep a calcium chloride tube ready to trap moisture from the air. Once I forgot and wound up scrubbing sticky white residue off everything nearby—not my best afternoon. Drop sulfuryl chloride into solvents slowly, never the other way around. I always keep a charged eye-wash and safety shower within five steps. Being able to yank yourself into water within seconds makes a real difference if something goes wrong.
Emergency Response and Training
Regular drills turn theory into instinct. Fire extinguishers and spill pillows look impressive on a checklist, but fumbling for them in an emergency costs lives. I’ve run drills that made folks notice they didn’t actually know where the nearest shower was. Every batch of newcomers gets hands-on practice in neutralizing spills and safely transferring small amounts. Reading a manual means little next to holding a mock bottle and running through the motions.
Looking Forward
Labs and workplaces benefit from talking about real incidents and sharing fixes. Companies that encourage reporting small mistakes—not just big ones—improve their record for everyone. Universities investing in regular equipment checks and honest timelines for replacing glassware help folks focus on science instead of putting out fires or nursing burns.
Getting to Know Sulfuryl Chloride
Sulfuryl chloride, with the formula SO2Cl2, brings a punch to the world of reactive chemicals. Its structure may sound simple at first, but in the lab or on the page, it tells a deeper story. I’ve watched students and young chemists get tripped up thinking it’s a cousin to sulfur dichloride. In reality, sulfuryl chloride packs in two oxygens and two chlorines all bonded to a central sulfur.
Each atom in SO2Cl2 takes a specific spot. Picture a sulfur atom at the center bonded to two oxygen atoms with double bonds and two chlorine atoms with single bonds. This tetrahedral structure matters a lot. Every corner houses its own group, leading to a molecule that's not exactly symmetrical. The double bonds to oxygen create areas of high electron density. This gives the molecule its punchy reactivity and also makes it a powerful chlorinating and oxidizing agent in industry and labs.
Why Care About Its Structure?
People often overlook how much a simple drawing on a blackboard can change safety, product design, or even product recalls. Knowing that sulfuryl chloride keeps its chlorines and oxygens in fixed spots helps chemists predict how it will behave. I remember one sticky summer day during a college internship, our team had to design a reaction protocol using sulfuryl chloride for making sulfonyl chlorides from alcohols. A rushed geometry mistake wrecked an entire batch of product and forced us to rethink glovebox safety. The layout of the SO2Cl2 molecule determines its caustic behavior with water—forming hydrochloric and sulfuric acids—and how it releases toxic fumes.
The molecule’s geometric setup also drives its use in making pesticides, dyes, and even for chlorinating polymers. Sulfuryl chloride doesn’t just swap its atoms for fun; it reacts strongly because of the electron-rich oxygens and the leaving group ability of chloride. Chemists dealing with this compound learn early to respect its power, keeping fume hoods running and goggles tight. In my own lab work, a moment of carelessness with SO2Cl2 led to a hasty evacuation, a lesson I’ll never forget.
Addressing Risks and Improving Safety
Working with sulfuryl chloride calls for serious safety measures beyond the minimum. Even small leaks mean instant corrosive gas, an experience no chemistry student forgets. Options like secondary containment, proper ventilation, and detailed safety training make a big difference. Firms and research groups should run regular drills so that everyone knows the risk and acts fast if trouble hits. Clear labeling also goes a long way—so many accidents start with a misread bottle on a crowded shelf.
Replacing sulfuryl chloride for some processes can cut risk, but sometimes there’s just no better substitute for its unique properties. For cases where alternatives work, choosing those options helps keep teams safer. When no substitute fits, tight operational controls and emergency planning matter most. Regulatory oversight, regular audits, and easy-to-understand safety data sheets help keep everyone on the same page, from students to seasoned chemical engineers.
The Takeaway: Knowledge Makes Chemistry Safer
With sulfuryl chloride, understanding its basic chemical makeup and three-dimensional structure does more than answer a test question. It shapes real-world lab safety, supply chain oversight, and industrial decisions. Risks jump when details get skipped. By leaning into the fine points—how sulfuryl chloride fits together at the atomic level—we set up the next generation to work smarter, safer, and with greater respect for the tools of our trade.
People and Chemistry Don’t Mix by Accident
Everyone in chemical handling circles has a story about a small oversight turning into a disaster. Years spent in labs and warehouses taught me that sulfuryl chloride isn't just another storage headache—it's a ticking clock. This stuff reacts fast with water, spews corrosive fumes, and gives off toxic gas with barely a nudge. A single spill once forced our whole floor to clear out for hours, after a novice stored it too close to a leaky rinse tank. Trust me—shortcuts will bite you on this one.
Humidity, Heat, and Human Nature
Sulfuryl chloride eats through skin and metal alike. It won’t wait for perfect lab conditions. Any bit of humidity lets it start breaking down, releasing noxious hydrogen chloride gas. One summer, a colleague stored a fresh drum in a building with poor air conditioning. By morning, rust streaks dripped from the cap. The clean-up crew wore double-layer gloves, and it still ended up bleaching their overalls. Storing it dry and cool is not just by-the-book—it’s about keeping people out of the ER.
Shelves along the back wall, far from sunlight, have always worked best in my experience. Windows and HVAC vents don’t mix with reactive chemicals. Even the most careful tech drops a wrench or drags a box too close eventually. That’s why I never put sulfuryl chloride higher than waist level. Tripping causes a bigger disaster than a broken thermometer.
Sealed Tight, Marked Clearly
I’ve learned to trust heavy-duty glass bottles, tightly sealed, with reinforced stoppers and PTFE liners. Sulfuryl chloride gnaws through plastics, and any tiny crack lets the fumes out. Labels must shout the hazard—eye-level, color-coded, big letters. More than one new worker has tried to grab it, thinking it was standard chlorinated solvent. A few seconds of confusion in the storeroom can end in months of paperwork, medical visits, or worse.
Segregation isn’t negotiable. Acids and bases cause chaos, but sulfuryl chloride and water? Pure catastrophe. During training, we drilled on keeping it on a separate tray, in a secondary container, far from sinks, hydrants, and even cleaning supplies. Some sites use locked cabinets with built-in trays for leaks—I always said yes to that expense. It’s much cheaper than scrubbing down an entire facility or rebuilding goodwill with your neighbors.
Emergency Plans Save Lives, Not Just Reputations
Every serious facility has a spill kit and a written response plan. I’ve had to use them. Respirator, heavy gloves, full apron, face shield—don’t skimp. Have eye wash stations unlocked and working. Talk through disaster scenarios out loud, before you need them. Nearly all sulfuryl chloride emergencies are totally preventable with common sense and strict routines. But shortcuts happen when pressure mounts, and no label or checklist can replace culture. Every chemist, lab manager, or warehouse worker needs to know that just a moment’s carelessness with sulfuryl chloride can cloud a career—or end a life.
It’s More Than Rules—It’s Respect
I’ve outlasted friends who shrugged off protocol out of boredom or bravado. The difference comes down to respect for the material, the team, and your own limits. Sulfuryl chloride doesn’t forgive—so those who store it with a plan, a backup plan, and an unwavering commitment to safety rarely have anything but stories and safe shelves to show for it.
Why Sulfuryl Chloride Exposure Demands Serious Attention
Sulfuryl chloride is no simple chemical to shrug off. It belongs to a group of compounds that command respect in the lab or plant. As a strong chlorinating agent, it gets put to work in chemical manufacturing, pesticides, and making pharmaceuticals. Mixing up with it, though, deserves real caution.
The Dangers of Coming in Contact with Sulfuryl Chloride
Nobody should underestimate the risks of this chemical. Inhalation, skin, or eye exposure all carry real danger. Breathing in sulfuryl chloride irritates the nose, throat, and lungs, triggering coughing, choking, chest pain, and even dangerous fluid buildup in the lungs if the situation turns ugly. Once it gets on skin or in eyes, pain and burns follow swiftly. I remember training for hazardous materials, and this compound stood out for how quickly it reacts with moisture—even sweat or tears—forming hydrochloric and sulfuric acids right on contact.
Spills get messy. Sulfuryl chloride releases toxic chlorine gas when it finds water or moist air. Chlorine isn’t just some sharp smell—it’s harmful and, at high enough concentrations, potentially fatal. People who think a mask or simple gloves will be enough put themselves at risk. Regular lab goggles and a dust mask do nothing for fumes or splashes.
First Aid: What Really Works in a Sulfuryl Chloride Emergency
Every second counts after an accident with sulfuryl chloride. Quick action can mean the difference between severe injury and a story to learn from.
Eye Contact
If sulfuryl chloride hits the eyes, speed is everything. Whoever is present should help the victim to rinse with clean, running water for at least 15 minutes—lifting eyelids but making sure not to rub. Personal experience from safety drills drives this point home: don’t reach for neutralizers, don’t use any bottle other than water. Only medical professionals can check the full extent of injury, so get help immediately.
Skin Exposure
Peeling off contaminated clothes comes first—don’t touch the fabric with bare hands. Flush the area with plenty of water for 15 minutes. People sometimes think brief contact isn’t so bad, but small spills can turn serious quickly. Skin absorbs the acid made by sulfuryl chloride, damaging tissue deeper than you’d expect. Send the victim to a doctor after rinsing.
Inhalation
If fumes have been inhaled, move the person straight into fresh air. Keep them still; rushing can make things worse. If breathing stops or becomes irregular, trained responders start CPR right away. Often, early symptoms—tight chest, wheezing, watery eyes—signal a need for urgent medical attention. Call emergency services before trying to drive the person anywhere.
Ingestion
Though rare, swallowing sulfuryl chloride is extremely serious. Never make someone vomit; dilute by giving water or milk if the person is conscious and able to swallow. Rushing to emergency care comes next.
Preventive Steps That Really Matter
Rely on practical safety basics learned through experience. Use proper chemical-resistant gloves, goggles with side shields, and a full-face shield when handling or decanting. Always keep work well-ventilated. Spill kits and safety showers should be close at hand—not tucked away in another room. Make sure everyone, from new hires to veterans, knows the emergency plan and how to use the eye wash station before an incident ever happens.
No one wants to face a sulfuryl chloride emergency. Still, understanding the risks and reacting the right way saves skin, lungs, and lives. For workplaces, staying prepared and respecting this chemical every single day proves more valuable than the fastest ambulance.
| Names | |
| Preferred IUPAC name | sulfuryl dichloride |
| Other names |
Sulphuryl chloride
Sulfuric chloride Sulfur oxychloride Sulfuryl dichloride |
| Pronunciation | /ˈsʌlfjəriːl ˈklɔːraɪd/ |
| Identifiers | |
| CAS Number | 7791-25-5 |
| 3D model (JSmol) | JSmol 3D model string for Sulfuryl Chloride (SO₂Cl₂): ``` S1 0.0000 0.0000 0.0000 O2 1.4012 0.0000 0.0000 O3 -0.7006 1.2142 0.0000 Cl4 -0.7006 -0.6071 1.1819 Cl5 -0.7006 -0.6071 -1.1819 ``` |
| Beilstein Reference | 1098721 |
| ChEBI | CHEBI:30169 |
| ChEMBL | CHEMBL1357 |
| ChemSpider | 35812 |
| DrugBank | DB11402 |
| ECHA InfoCard | 03c7d516-a05c-4b23-aef9-b3e50b1a2261 |
| EC Number | 016-102-00-8 |
| Gmelin Reference | 778 |
| KEGG | C01749 |
| MeSH | D013440 |
| PubChem CID | 24814 |
| RTECS number | WS5600000 |
| UNII | Q508N1KIWZ |
| UN number | UN1827 |
| CompTox Dashboard (EPA) | DTXSID5020707 |
| Properties | |
| Chemical formula | SO2Cl2 |
| Molar mass | 118.97 g/mol |
| Appearance | Colorless to pale yellow fuming liquid |
| Odor | Pungent odor |
| Density | 1.67 g/cm³ |
| Solubility in water | Decomposes in water |
| log P | -0.48 |
| Vapor pressure | 19.2°C (1400 mmHg) |
| Acidity (pKa) | -2.0 |
| Basicity (pKb) | -3.70 |
| Magnetic susceptibility (χ) | -40.6·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.509 |
| Viscosity | 1.098 mPa·s (20 °C) |
| Dipole moment | 0.97 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 247.6 J⋅mol⁻¹⋅K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -512.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -296 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | No ATC code |
| Hazards | |
| Main hazards | Toxic if swallowed, inhaled or in contact with skin; causes severe burns and eye damage; releases toxic gases upon contact with water or moisture. |
| GHS labelling | GHS02, GHS05, GHS06 |
| Pictograms | GHS05,GHS06 |
| Signal word | Danger |
| Hazard statements | H301 + H314 + H331: Toxic if swallowed. Causes severe skin burns and eye damage. Toxic if inhaled. |
| Precautionary statements | P210, P220, P260, P273, P280, P303+P361+P353, P304+P340, P305+P351+P338, P307+P311, P363, P405, P501 |
| NFPA 704 (fire diamond) | 3-0-2-W |
| Autoignition temperature | 230 °C |
| Lethal dose or concentration | LD50 oral rat 180 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral-rat LD50: 180 mg/kg |
| NIOSH | NIOSH: WX8800000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) of Sulfuryl Chloride SCl: 1 ppm (5 mg/m³) |
| REL (Recommended) | 70°F |
| IDLH (Immediate danger) | 20 ppm |
| Related compounds | |
| Related compounds |
Chlorosulfuric acid
Sulfur dichloride Sulfur monochloride Thionyl chloride Sulfuryl fluoride Sulfur dioxide Sulfur trioxide |
