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Few chemistries have woven themselves so deeply into daily routines, global industries, and scientific puzzles as organosulfur compounds. Ancient Egyptians used incense brimming with organic sulfur, and by the Middle Ages, alchemists tinkered with sulfurous oils. In the industrial era, factories pumped out thiols, sulfoxides, and sulfones for everything from dyes to explosives. Chemistry books detail the stench of mercaptans, a nature-approved warning sign, but most stories stop at the nose. Having spent years in a research lab haunted by the aroma of onions and garlic, I’ve seen how quickly conversations turn when sulfur compounds come to the table—either you’re caught by surprise, or you’re hooked on their possibilities. The infamous “rot” smell of hydrogen sulfide often keeps researchers humble, and lab stories about “clearing the building” after a failed synthesis reinforce just how memorable and potent these compounds can be. Yet their reach goes far beyond warning odors. Sulfur-containing molecules sit inside medicines, crop protection chemicals, rubber, batteries, and, of course, the garlicky zest in a home-cooked meal. History shows that while folk treatments using garlic or mustard embraced sulfur long before chemists extracted their secrets, only in the past century have we mapped the sheer versatility of this chemical clan.
Opening a medicine cabinet, you’ll likely spot products whose effectiveness comes from organosulfur compounds. The anti-inflammatory punch in sulfa drugs, the power in anti-epileptics, or the resilience built into vulcanized rubber all rely on sulfur atoms tucked into organic frameworks. In my teaching days, discussing how “skunk spray” or natural gas warning agents work pulled in even the most distracted students—organosulfur compounds provide some of the most visceral, memorable experiences both in the wild and our built environments. Glance at chemical industry statistics, and you’ll see millions of tons of organosulfur chemicals produced annually, especially for the tire industry, pharmaceuticals, and crop protection. The profiles of thiols, sulfides, and sulfoxides—each with different smells, reactivities, and safety profiles—lead to applications as diverse as pest management, vapor phase corrosion inhibitors, and very specific flavorings. Household cleaning agents sometimes use sulfones, and winemakers measure sulfur content in their products far more than the average consumer suspects.
Sulfur atoms march to a different beat than their oxygen cousins. That little difference in atomic mass and electron count means organosulfur compounds display quirks across the board—boiling points, odors, solubilities, and reactivities. Thiols, for example, tend to have high volatility and persistently sharp, unpleasant odors at trace levels. Sulfides often show up as stable oils with lower polarity compared to their oxygen analogs. Having wrestled with hydrophobic sulfides in phase transfer reactions, I can say they rarely behave as expected. Many organosulfur compounds react easily with oxidants—sometimes so fast they challenge chemical intuition. This trait makes them valuable in antioxidant applications but introduces hazards when mixed with strong acids or oxidizers. Variability in melting and boiling points stems from subtle changes in molecular shape and intermolecular forces, which becomes painfully evident when trying to purify these compounds by distillation. Even physical appearance, from oily liquids to needle-like crystalline solids, hints at just how broad the family of organosulfur molecules can be.
Synthetic routes for organosulfur compounds often seem like organic chemistry’s ultimate test of patience and creativity. Typical lab synthesis uses reactions between alkyl halides and potassium thiolate salts, or employs sulfonation through concentrated sulfuric acid. Scaling these up to commercial levels introduces a new level of caution—safety procedures become gospel, and labeling rules intensify. Reach for laboratory catalogs and you’ll see compound names like “diethyl sulfide” or “dimethyl sulfoxide (DMSO)” stamped on barrels with highly visible hazard markings, including “flammable,” “toxic,” or “harmful if inhaled.” In my experience, label discipline isn’t just regulatory—it’s about protecting everyone working with these volatile or stinky substances. Consistent, clear labeling, with full chemical identifiers, keeps confusion low and safety high. Reports of close calls or actual poisonings always remind researchers that even familiar chemicals, when misused or misidentified, can do real harm.
Organic chemists seem to develop a sixth sense for sulfur’s behavior. Reactivity patterns differ from nitrogen or oxygen compounds, sometimes dramatically. For example, oxidation of a thioether often leads to a sulfoxide or sulfone without much effort, a reaction harnessed industrially for synthesis of solvents or intermediates. Sulfonation, Swern oxidations, and S-alkylation reactions pepper research notebooks, and learning the “smells” of the process helps catch mistakes early—there’s nothing quite as distinct as over-oxidized thiol. Beyond this, trivial and trade names abound: “mustard gas” hides as sulfur mustard, “DMSO” as a pharmaceutical carrier or cryoprotectant, “methionine” as an essential amino acid feeding into animal health. Reversible and irreversible modifications of organosulfur scaffolds fuel patents and keep chemical producers scrambling for new, smarter ways to tweak old molecules. The variety of alkyl, aryl, sulfonyl, and oxidized or reduced forms opens the floodgates for medicinal chemists and material scientists searching for that next big breakthrough.
Sulfur compounds take safety training from chore to necessity. Even seasoned bench chemists have stories about accidental exposure—lachrymation, dizziness, or the embarrassment of trailing stink through an entire building. Industry standards for ventilation, personal protective equipment, and storage have grown more stringent over decades, driven less by regulatory fines and more by hard-learned lessons passed down the grapevine. Proper gloves, tight-sealing bottles, and training to recognize leaks protect workers, but also lessen the odds of chemical escapes. Real-world incidents, such as accidental thiol releases from chemical plants, have forced revisions to emergency response protocols. Workers now learn detailed actions for chemical containment and decontamination, and chemical labels no longer shy away from stating the risk of chronic effects or environmental persistence. There’s a quiet camaraderie among those who have “taken one for the team” in a sulfur lab, and each scare sharpens the community’s respect for operational discipline.
Scratch any major industry, and you’re bound to see the fingerprints of organosulfur chemistry. From rubber vulcanization—where cross-linking by sulfur transforms sticky natural rubber into tough, durable material—to antimicrobial agents in agriculture and pharmaceuticals, sulfur finds ways to add value at every step. In batteries, sulfur-based cathodes hint at the future of high-energy storage, promising lighter and cheaper alternatives to traditional lithium-ion setups. Pesticide formulas have long relied on the selective toxicity of certain organosulfur agents, often attracting controversy but also playing a major role in global food security. Prominent medications, such as antibiotics and anti-inflammatory drugs, source their effectiveness from sulfur atoms that alter biological processes. On the food science front, molecules like allicin from garlic not only give flavor but also fight microbes and reduce spoilage. The simple act of peeling an onion reveals how chemicals like syn-propanethial-S-oxide truly have the power to affect physiology—tears in the kitchen trace back to subtle differences in sulfur chemistry. As consumer awareness of food additives and environmental issues grows, researchers are being pushed to find greener ways to deploy these compounds.
Innovation windows open widest where chemistry, biology, and materials science overlap. Research groups continue to unlock the medical potential of sulfur compounds, inspired by findings that link dietary sulfur intake to cardiovascular health or by discoveries at the heart of antibiotic resistance. My own experience in developing novel sulfonylurea pharmaceuticals hammered home both the promise and the frustration of this chemistry—each promising lead often carries a risk of toxicity or instability, demanding smarter formulation and delivery systems. Fuel research aims to harness sulfur’s unique electron properties for batteries with higher capacity and greater resource security, a real game-changer if it pans out. Environmental scientists now scan water and soil for residual thiols, mercaptans, and sulfonated surfactants, driving policy changes and tighter controls. Patents filed each year point to ever more targeted and efficient uses for these compounds, in areas as unexpected as cancer therapy or new forms of materials for electronics. As research budgets fluctuate and regulatory demands tighten, those working in this space must stay nimble, balancing risk with promise.
Persistent caution is a defining trait in handling organosulfur compounds, for good reason. Acute and chronic toxicity range from mild irritation, like the tears from kitchen onions, all the way up to incapacitating effects in the case of industrial accidents. Take a lesson from history: “mustard gas,” a particularly nasty sulfur war agent, changed how the world thinks about chemical weapons. In milder but still serious cases, some organosulfur pesticides threaten aquatic life and bioaccumulate, leading to regulatory bans or phaseouts over time. Human toxicity studies point to organ damage, nervous system effects, or allergic reactions depending on dose, formulation, and route of exposure. In my graduate lab, accidental skin contact with concentrated thiol taught me the hard way never to underestimate risks. Modern toxicology works to pinpoint safe exposure thresholds, and new guidelines arrive every year reminding users of both direct and environmental dangers. Public communication on risks and proper handling remains one of the biggest challenges for both industry and regulators, especially given the stigma attached to chemical “smells.” Educating communities about the difference between nuisance and hazard, and making safety data publicly available, forms a critical, ongoing project in both academic and industrial settings.
Few chemical families stretch further into the future than organosulfur compounds. Their unique chemistry fuels breakthroughs in clean energy, smarter medicines, and sustainable agriculture, even while regulatory pressures and environmental concerns raise new hurdles. Explosive growth in green chemistry highlights the ongoing search for less-hazardous synthesis and cleaner degradation pathways. Reducing reliance on organosulfur pesticides, finding alternatives that preserve yield without risking runoff or groundwater contamination, occupies public and private researchers alike. Battery and fuel cell developers keep one eye on the periodic table and another on the ticking clock of resource insecurity, banking on sulfur’s abundance and versatility. In medicine, researchers probe deeper into sulfur’s mysterious roles in biology—parsing out antioxidant effects, signaling roles, and mechanisms of action for old and new drugs. My time tracking the impact of sulfur-bearing metabolic byproducts suggests we’ve only scratched the surface—the next decades will likely reveal entirely new application frontiers, and risks we haven’t yet imagined. So, as much as the compounds themselves have been around since the dawn of chemistry, our true understanding and control over organosulfur chemistry stands on the edge of its own breakthrough moment.
From the sharp bite of garlic to the mousey aroma of truffles, sulfur fills our senses in the kitchen. Organosulfur compounds, the family that brings sulfur and carbon together, go far beyond flavor. They hold their own in medicine, agriculture, and even big industry.
Growing up, I remember the yellow bottle of sulfa drugs in my grandmother’s medicine cabinet. These compounds changed the world, pushing back bacterial infections before penicillin became widely used. Sulfonamides, a class of organosulfur drugs, broke ground for antibiotics. Even now, some folks rely on these medications when allergies or resistance get in the way of newer treatments.
Oncology turns to organosulfur as well. Compounds like busulfan step in to help manage certain leukemias. Allicin from garlic, another organosulfur, gets credit in early research for possible cancer-fighting traits. Science isn’t done exploring these options.
Sulfur feels old-fashioned, but organosulfur compounds still protect crops in big ways. Fungicides with sulfur at their core knock out powdery mildew and rust on grapes, apples, and more. I spent summers as a teen walking fields for a neighbor who farmed wine grapes. Sulfur’s pungent smell stuck in my clothes long after, but so did the lesson: without this element, the harvest would’ve suffered.
Crops face threats that change each season, and chemists keep developing new organosulfur molecules to hit stubborn weeds and fungi that move past older sprays.
Car tires stay flexible thanks to sulfur’s knack for linking rubber molecules, a process called vulcanization. Without this, tires couldn’t handle heat or wear from daily driving. I watched a tire shop patch a hole for my uncle, and the smell of hot rubber carried with it the importance of these chemical bonds.
Petroleum refining leans heavily on organosulfur chemistry as well. Refineries crack open petroleum molecules, then remove sulfur to meet clean air rules. More than that, organosulfur helps make things like pesticides, dyes, and even detergents that keep homes and clothing clean.
Onions, garlic, and cabbage owe their bite and beneficial effects to their sulfur-based molecules. These foods keep more than flavor on the table—they offer antioxidant and heart-friendly effects. Anyone who’s chopped an onion knows just how much of an impact tiny chemical differences can have on daily life, turning bland meals into something better.
Some of these compounds bring health and environmental worries. Pesticides drift from fields, drug residues wind up in drinking water, and sulfur compounds released at plants can smell up neighborhoods. Regulators and scientists keep searching for lower-risk, more targeted products. Industry also looks for ways to recycle sulfur and trap unwanted emissions before they reach the air.
Cleaner production methods attract attention now. Green chemistry—using plants or microbes—has begun to shape today’s research. This reduces harmful waste and puts safer products on the market.
Organosulfur compounds deserve a closer look, not just from scientists but all of us. From medicine and farming to city streets and kitchens, sulfur’s fingerprints show up everywhere. Staying curious about these building blocks pushes us to question where our goods come from and what it takes to make daily life possible. By understanding these hidden connections, we make wiser decisions about what we grow, eat, and use.
Spend any time looking at chemistry in foods or the environment, organosulfur compounds pop up all over the place. These molecules carry at least one sulfur atom attached to carbon. They're responsible for the unmistakable aroma of garlic, onions, and even the skunk’s infamous spray. People have used them for centuries, from medicine to agriculture. Yet, reading about "sulfur" can make toxicity concerns float to the top of your mind.
Eating garlic isn’t toxic for most folks—actually, garlic’s main compounds, allicin and diallyl disulfide, help with cholesterol and may lower blood pressure. Broccoli, Brussels sprouts, and other cruciferous vegetables pack glucosinolates, another group of these compounds, which help the body clear out some carcinogens. Researchers link these foods with lower risks of certain cancers, showing that organosulfur molecules can work wonders in the right dose or context.
Some organosulfur compounds have powerful antimicrobial properties. Hospitals rely on drugs like sulfonamides, a class of antibiotics with sulfur in their structure. These drugs fought bacterial infections long before penicillin came along, and they remain crucial against antibiotic-resistant bugs.
Industry also leans hard on organosulfur molecules. Additives in fuels, pesticides on crops, rubber vulcanization—these all need sulfur-containing chemicals. Methyl mercaptan, for example, helps give natural gas its odor so leaks get noticed fast. But not every application comes risk-free.
Sulfur atoms have a talent for forming strong bonds with metals. That’s why many organosulfur compounds pop up in heavy industry pollution. Mining and chemical production sometimes release hydrogen sulfide or carbon disulfide, both organosulfur gases, into the air or water. Breathing hydrogen sulfide, even in low doses, irritates eyes and lungs; higher doses shut down breathing and become lethal in minutes. Carbon disulfide, used in some rayon production, harms the nervous system if inhaled for long periods.
Then there’s the issue of certain pesticides. Organosulfur compounds like malathion or parathion can disrupt enzymes in the nervous system, which can cause seizures or even death at high exposures. Farmworkers spraying crops day in and day out risk headaches and other symptoms if they don’t wear the right protection. In many countries, health regulations and safety equipment help lower the danger, but accidents still happen.
My background in agriculture brought real encounters with sulfur-based fungicides. Some afternoons, the fields reeked like rotten eggs. The label warnings got my attention more than the smell—long sleeves, gloves, and a mask became non-negotiable gear. I saw what happened when those warnings got ignored. Rashes, eye pain, and breathing problems are not rare after accidental overexposure. Local clinics backed that up: reports of chemical exposure spike during spraying seasons.
Peer-reviewed studies show links between long-term organosulfur exposure and health issues, especially in poorly regulated work environments. The National Institutes of Health, for instance, has documented cases of chronic neurological symptoms in workers exposed to certain sulfur pesticides. Research keeps tracking accidental releases from chemical plants, with clear evidence of increased respiratory and cardiovascular risks in affected areas.
Practical steps go a long way. Strong oversight, transparent chemical labeling, and investment in less toxic alternatives help safeguard workers, residents, and the planet. Farmers and industrial workers should have easy access to reusable protective clothing, and emergency response teams need clear reporting protocols for spills and leaks. People in agriculture and industry—plus those living nearby—should know what’s in the air and water around them.
The story with organosulfur compounds isn’t simple. Some are friends—the foundation of good meals and medicine. Others threaten health or the environment when they’re mishandled. Fact-based education, careful monitoring, and personal protection keep the risks in check and let these useful but sometimes dangerous compounds do more good than harm.
Most folks recoil a bit at the smell of onions or garlic and don’t realize they’re getting a good whiff of organosulfur compounds. Slice an onion and the gas making your eyes water is actually syn-Propanethial-S-oxide, a mouthful of a word that signals your kitchen is now a chemistry lab. If garlic goes into the pan, allicin starts breaking down, filling the air and your meal with both health benefits and a sharp, biting aroma. Doctors and nutritionists, backed by many peer-reviewed studies, point to these same compounds for their antibacterial and potential heart-protective qualities.
Dimethyl sulfide has a reputation for giving decaying cabbage and some ocean air its strong odor. It may not sound flattering, but this compound signals everything from safe seafood to environmental changes. Students in the chemistry lab might be told to handle thiols with care. Ethanethiol, for example, is added to natural gas not for chemistry’s sake, but as a safety device. Its intensely foul scent warns of leaks long before danger strikes.
Lots of modern medications start with a dash of sulfur. Sulfa drugs, like sulfamethoxazole, brought hope to a world battered by bacterial infection in the twentieth century. Later, doctors started prescribing captopril for high blood pressure, and there’s a unique taste if you check: a sulfur atom in its molecular skeleton. Chemists try to improve these medicines, using both clinical trials and a good bit of serendipity.
Rubber tires owe some of their toughness to vulcanization, a process involving sulfur and, in some cases, organosulfur accelerators such as mercaptobenzothiazole. Factories use these not for thrills, but to make sure your tires grip the road instead of wearing out too soon. In refineries, scientists face the task of removing thiophene and other sulfur compounds from oil, helping to cut down on air pollution and acid rain. Keeping sulfur in check makes a real difference, especially for communities near industrial centers.
Not all stories about organosulfur compounds stay positive. Cities can face odor issues when hydrogen sulfide—one sulfur compound—escapes from sewers or industry, quickly causing headaches or worse. The World Health Organization highlights links between high-long term exposure and respiratory issues. Scrubbing technologies stand ready, but enforcement and maintenance take money and commitment at every level.
Learning to handle organosulfur compounds safely demands both education and regulation. Proper personal protective equipment, exhaust systems in research labs, and strict emissions standards in industry all protect health. A public informed about which household cleaners or foods contain organosulfur compounds can use them with less risk. Local governments, employers, and households all play a part, making smart use of old chemistry lessons and new safety data.
Anyone who has cracked open a bottle of thiols or sulfoxides knows that unmistakable, nose-wrinkling punch. In the lab, a few drops spilled on a glove or bench linger long after, testing both patience and safety routines. Organosulfur compounds go beyond inconvenience: some are toxic, reactive with air, or flammable. A safety slip can spoil a lab’s air—and much more. Their volatility and chemical reactivity deserve respect, not just from chemists but from those in industry, storage, and transport.
Years spent working with compounds like dimethyl sulfide and thiophenol have taught me that a lot of risk gets managed with the right container and storage location. Glass bottles with Teflon-lined caps usually work best. Metal containers often mean trouble—sulfur compounds can eat through some metals or even react. I’ve seen cases where careless choice of container led to sour-smelling leaks, sometimes in chemical storerooms shared with oxidants—never a good idea.
A dry, cool cabinet, away from sources of ignition, minimizes risk. Moisture is trouble: many organosulfur chemicals break down in the presence of water or produce hydrogen sulfide, a highly toxic gas. Storing these chemicals in a dedicated flammables cabinet is smart, especially if you work in a warm or humid climate. Keeping them away from acids and oxidizers should be a fixed rule—these combinations invite dangerous reactions. I’ve set a habit of using color-coded labels and checklists, after seeing too many close calls from simple mix-ups.
Not all organosulfur compounds react the same way to light and oxygen, but plenty oxidize or degrade faster than people think. Some emit fumes on slow breakdown, irritating eyes and lungs. Tight-sealing caps or septa help a lot. For very sensitive chemicals, storing under inert gas (like nitrogen or argon) makes a difference. One chemistry professor I worked with showed me a double-sealing method: parafilm and Teflon—a trick that saved a few expensive reagents during summer power outages.
Those who regularly store organosulfur compounds in clear bottles under bright lab lights risk more than odor buildup; photodegradation can lead to loss of purity or unpredictable products. Amber glass or a closed cabinet keeps shelf life long, and headaches rare.
Poor storage doesn’t just hurt scientists. Contaminated shipments reach manufacturing floors. Odors leak into shared building spaces. Waste handling staff face unexpected exposures. A spill can trigger regulatory nightmares and real health problems.
The CDC and OSHA offer clear guidance—they’ve documented serious incidents linked to improper storage. Following their recommendations saves money, time, and sometimes lives. Training new staff on safe practices is as important as any fire drill. Retelling cautionary tales—like the time an open bottle set off an entire building’s H2S alarms—sticks with people and keeps safety at the top of mind.
Collaboration makes a difference. A well-organized chemical inventory, regular checks of seals and containers, and clear signage for storage zones help everyone. Asking vendors about recommended packaging and expiry dates stops problems before they start. Developing spill and exposure plans means you don’t panic when something goes wrong—you act quickly.
Organosulfur compounds aren’t going away—they power industries from pharmaceuticals to agriculture. Treating them with caution and planning isn’t just good lab etiquette. It respects people’s health, supports regulatory compliance, and protects the value of these important but sometimes underestimated molecules.
Anyone who’s ever cracked open a bottle of thiol knows the unmistakable punch of rotten eggs. Organosulfur compounds have a way of introducing themselves. These aren’t substances to wave around indoors or handle with a quick sniff. The truth is, stink is just the warning sign. Some sulfur-containing chemicals, especially volatile ones, can harm far more than your nose if handled without care. Toxic effects range from mild headaches to organ damage. Some, like dimethyl sulfide, catch fire as easily as gasoline. A few can even knock out your sense of smell long before you realize the air in the lab has reached danger levels.
I can’t count the number of times someone thought latex gloves offered a shield to anything in a bottle. Unfortunately, organosulfur molecules can slip through more than a few glove materials. Not all gloves hold up; nitrile works better, but even those start breaking down with repeated use or after a splash. Wash skin quickly if anything spills—soap and water, right away, no waiting for the safety officer.
Good air movement changes the game. Fume hoods aren’t just big boxes taking up space; they draw away hazardous vapors before you ever know a spill happened. I once worked in a place that skipped ventilation fixes longer than they should have. One forgotten spill, and several people left the lab with irritated lungs. Keep that sash down so the air flow stays strong, and never let a job expand beyond the fume hood. Some organosulfur gases weigh more than air and sink low—ventilation above and below helps.
Safety glasses block splashes, but organosulfur compounds can burn without ever touching the eye’s surface. Vapor-proof goggles give far better protection than open glasses. In a real-world emergency, a proper eyewash station can mean the difference between a temporary sting and a long-term injury.
Spill kits belong close at hand, but there’s more to cleanup than throwing absorbent pads on a puddle. Many of these compounds react with water or simple cleaning products, sometimes producing worse fumes. I’ve watched someone turn a small mess into a full-scale evacuation by using the wrong neutralizer. Keep incompatible chemicals separated, especially oxidizers or acids, which love to react with sulfur-containing organics. Companies like DSM and Merck label storage cabinets and segregate organosulfur bottles for a reason—one mistake sends everyone home early, sometimes to the hospital.
Book learning gives a foundation, but there’s nothing like seeing proper handling in action. New hires watch and practice under supervision—not just because the rules say so, but because experience matters when snapping off a stuck cap or cleaning a sticky transfer line. Management needs regular drills, not just once when someone starts. In a real spill or fire, calm only comes from muscle memory.
Plenty of mistakes happen when team members feel pressured to look tough or act like they know it all. No one has all the answers, and rules change as new data comes out. A safe lab encourages people to stop and ask: “Is this the right glove?” or “Do I need the full-face shield right now?” Making safety part of everyday conversation works better than any poster or warning sign.
Regulations tell only part of the story. Regular monitoring, rotating training, and keeping open lines between researchers and safety staff keep hazards low and productivity high. Simple steps—fresh gloves, working fume hoods, regular air testing—carry more weight than any compliance checklist. Organosulfur compounds make life-saving drugs, dyes, and agrochemicals, but they don’t forgive shortcuts. For anyone working with them, safety only grows more important the more you learn.
| Names | |
| Preferred IUPAC name | organosulfanes |
| Other names |
Thiocompounds Organosulfides |
| Pronunciation | /ɔːˌɡæn.oʊˈsʌl.fər ˈkɒm.paʊndz/ |
| Identifiers | |
| CAS Number | 68259-80-9 |
| Beilstein Reference | IV/9 |
| ChEBI | CHEBI:36653 |
| ChEMBL | CHEMBL222 |
| ChemSpider | 21548 |
| DrugBank | DB03602 |
| ECHA InfoCard | 03f7c36a-85ef-49d2-951a-bde3a814b9ef |
| EC Number | 2.2.1.1 |
| Gmelin Reference | C10 |
| KEGG | map00997 |
| MeSH | D010351 |
| PubChem CID | 7047 |
| RTECS number | WN2636000 |
| UNII | J3W928RDJ9 |
| UN number | UN2810 |
| Properties | |
| Chemical formula | R-S-R' |
| Molar mass | Varies depending on the specific compound |
| Appearance | Colorless or pale yellow liquids or solids with a characteristic odor |
| Odor | Pungent |
| Density | 1.00 g/cm3 |
| Solubility in water | slightly soluble |
| log P | 4.27 |
| Vapor pressure | <0.01 hPa (20°C) |
| Acidity (pKa) | 7-11 |
| Basicity (pKb) | 3 – 9 |
| Magnetic susceptibility (χ) | -5.5×10^-6 |
| Refractive index (nD) | 1.525 |
| Viscosity | 4.8–5.2 cP |
| Dipole moment | 1.613 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | Organosulfur Compounds: 302.2 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -93.13 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1230 to -2590 kJ/mol |
| Pharmacology | |
| ATC code | A16AX |
| Hazards | |
| GHS labelling | GHS02, GHS05, GHS07, GHS08 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Precautionary statements | P261, P280, P305+P351+P338, P337+P313 |
| NFPA 704 (fire diamond) | 2-3-0 |
| Autoignition temperature | AUTOIGNITION: 249 °C |
| Lethal dose or concentration | LD50 (oral, rat): > 5,000 mg/kg |
| LD50 (median dose) | LD50 (median dose): 260 mg/kg (oral, rat) |
| NIOSH | RN8780000 |
| PEL (Permissible) | 15 mg/m3 |
| REL (Recommended) | 0.1 mg/m3 |
| IDLH (Immediate danger) | IDLH: 50 ppm |
| Related compounds | |
| Related compounds |
Thiols Thioethers Sulfoxides Sulfones Sulfonic acids Sulfonamides Disulfides Sulfides |
