Monosulfur silane has roots grounded in the growth of organosilicon chemistry, which started picking up pace in the early 1900s. Before the world understood the power of silicon-based chemistry, folks relied on simple silica compounds—think glass, ceramics, even early sealants. By the 1940s and 50s, researchers looking to toughen rubbers and fine-tune chemical bonds experimented with silanes. Some Eureka moments emerged in German and U.S. research labs; they found that by introducing sulfur atoms to silane molecules, new reaction pathways opened up. Chemists working on tire technology and advanced adhesives spotted the benefits early, paving the way for large-scale production. These little tweaks to the molecule turned monofunctional silanes from mere curiosities into fundamental building blocks for materials science and rubber compounding.
In basic terms, monosulfur silane is a silane molecule holding a sulfur atom. Most commonly, it looks like SiH3-SH or SiR3-S-R’, where an organic group is linked to silicon, and that sulfur link changes everything. Companies offer it in liquid or sometimes low-melting solid form. It’s far from an everyday household name, but show up in the supply chains for rubber, plastics, cables, and construction sealants, usually under product names from Silquest, Momentive, or Evonik. These aren’t products you ever buy at the store, but the people making tread compounds or solar panel laminates pay close attention to the details. Synonyms in trade catalogs vary, including terms like “sulfur-functional silane” or “mercaptosilane.”
Monosulfur silanes generally feature a pungent, mercaptan-like odor, warning you of reactive sulfur. These molecules are clear to pale yellow, with a slightly oily texture in pure form. Unlike simple silanes, adding the sulfur atom increases chemical reactivity. Melting and boiling points fluctuate, depending on the exact organic groups attached, but most monosulfur silanes volatilize at moderate temperatures, above 150°C. With moisture, monosulfur silane reacts, producing hydrogen sulfide gas and silanols, and this moisture sensitivity shapes its storage and handling. Reactivity with bases and oxidizers also shows up prominently—splitting out sulfides or creating gels. If you work with rubbers and resins, you’re looking for tight control over these chemical reactions, since a little too much heat or the wrong mix of ingredients can spoil an entire batch.
Buyers and formulators scrutinize details like purity, percentage sulfur, silane content, and residual chlorosilane or alcohol, depending on the batch’s route of synthesis. Specifications may list a CAS number like 4420-74-0, with concentrations described down to the half-percent in technical datasheets. Labels warn about hydrogen sulfide release, skin and eye irritation, and the hazards of inhalation. Bulk packing comes in steel drums or tightly sealed glass bottles for lab use, since the product can leak volatile odors and degrade if care slips. In my experience, product inspection teams pay close attention to expiry dates, looking for cloudiness or hints of crystallization that might signal hydrolysis or worse.
Production workflows for monosulfur silane take root in two main approaches: direct synthesis from alkoxysilanes and sulfur, or hydrosilylation with mercaptans under a catalyst. One old-school method involved bubbling hydrogen sulfide over chlorosilane compounds, but the resulting mess of byproducts put folks off. Smarter routes involve platinum-catalyzed hydrosilylation or thermal reaction of trialkoxysilane with thiol compounds. These are batch or continuous-reactor processes, designed to minimize moisture and oxygen exposure. Each route creates challenges: deal with byproduct management, prevent catalyst poisoning, or keep the end product stable as it travels to the next factory. My conversations with process engineers echo the same refrain—consistency matters, and even a slight slip means a shipment gets sent back, piling up delays.
Once you have a batch of monosulfur silane, its chemistry shines brightest in coupling and crosslinking reactions. The silane end likes to attach to glass, silica, metal oxides, or even carbon black, forming strong bonds. Meanwhile, the sulfur end grabs onto natural or synthetic rubber chains. This dual personality lets rubber makers reinforce tires and elastomer goods at the molecular level, giving more strength, abrasion resistance, and controlled elasticity. For plastics, monosulfur silane allows for surface modification, improving adhesion or moisture resistance. Other chemists tweak the base molecule, replacing organic groups with bulkier or more reactive types, squeezing out new properties for custom uses. In lab experiments, these modified forms enter specialty fields—delivery of other functional groups, surface coatings for electronics, and even anti-fouling maritime paints.
Monosulfur silane appears under labels such as “mercaptosilane,” “thiol silane,” or “sulfur silane coupling agent,” depending on supplier or the functional group’s location. In catalogs, you spot names like Si-69, MPTMS (mercaptopropyltrimethoxysilane), or even brand-specific codes. Some specific chemical synonyms include 3-mercaptopropyltrimethoxysilane and similar derivatives. Users juggling dozens of silanes in inventory see these labels and spot the sulfur function right away, since no other silane brings that rotten-egg scent or the reactivity you need for tire compounding.
Safety standards around monosulfur silane ask for respect. Breathing the vapors or touching the liquid can irritate skin, eyes, and lungs. Long exposure, especially in a closed space, builds up hydrogen sulfide and brings genuine toxicity risk—deadly in high enough doses. The industry relies on ventilation, tight seals, full-face respirators, neoprene gloves, and sometimes scrubbers. Operators score regular training on spill cleanup and emergency procedures, not just OSHA compliance checkbox exercises. Adherence to safety data sheets and GHS labeling help avoid confusion, though product names across companies sometimes muddy the waters. Even with safety gear, batch sampling requires focus, since leaks or unplanned reactions can create dangerous byproducts or fires.
Monosulfur silane earns its pay in the rubber industry, especially for tires, industrial hoses, and vibration-damping parts. Tire performance—grip, rolling resistance, wear—links right back to how well the silane bonds silica to rubber. In cable manufacturing, this compound helps tie insulation layers to conductors, cutting down on delamination. In adhesives and sealants, that sulfur group helps stick to metal or glass, boosting weather resistance and longevity. Some coatings and paints add low levels of monosulfur silane to improve adhesion and durability, especially in harsh outdoor environments. More recent developments target solar panel encapsulation, where the compound supports strong, long-lasting bonds under changing temperatures.
Research teams continue pushing monosulfur silane boundaries. In university and corporate labs, the search goes on for improved versions with lower toxicity, higher reactivity, or more selectivity in coupling. Recent publications focus on tuning the organic “tail” for better performance in tires or looking for green chemistry options that reduce emissions during manufacturing. In academic circles, researchers publish studies on silane-modified nanomaterials, merging rubbers and ceramics, or exploring recycling techniques that break the sulfur-silicon bond without heavy waste streams. I’ve seen research groups at conferences trading results on silane compatibility in bioplastics, or inventing catalysts that lower the reaction temperature.
Monosulfur silane’s greatest risk comes from its breakdown products. Hydrogen sulfide can kill in minutes, forcing safety reviews every time a plant adopts a new silane. Recent government and academic studies suggest chronic exposure increases risks of respiratory issues and sensitization. Industry-funded toxicology research tests new derivatives for skin absorption and mutagenicity, seeking lower-toxicity alternatives while meeting the same technical features. Animal studies and in vitro tests on cell cultures help map out safe handling levels, but real-world incidents push companies to add extra scrutiny, double containment, and better detection systems. Ongoing work looks into biomonitoring for exposed workers, and improved waste management to keep sulfides out of water tables.
Looking forward, monosulfur silane won’t lose its place in high-performance rubber and composite processing, but the game is changing. Sustainability pressures, both regulatory and consumer-driven, are driving investment in “greener” manufacturing methods. Research now aims at recycling silane-containing rubber, converting waste streams into reusable chemicals, and even sourcing silicon from renewable silica. There’s a push to lower risk by redesigning molecules for reduced toxicity, swapping hazardous production chemicals for safer ones, or switching to closed-loop systems. Digitally tracked product supply chains and AI-assisted quality controllers are beginning to take guesswork out of production batches. For engineers and researchers, monosulfur silane still holds promise for untapped fields—smart coatings, medical-device adhesives, or flexible electronics. The road ahead isn’t without roadblocks, but the blend of chemistry knowhow and risk management will shape what monosulfur silane does for the next hundred years.
Ask anyone in tire manufacturing or the rubber industry about what makes their products stick together and last longer, and they’ll probably mention silanes at some point. Monosulfur silane stands out here. In making tires, it forms chemical bonds between the rubber and fillers like silica. These bonds matter. Good bonding means stronger, more flexible tires and less risk of blowouts or early wear.
Living in a city where tire replacements aren’t cheap, I’ve seen the benefits myself. Car owners want tires that handle wet roads and high heat. Monosulfur silane helps meet both needs. It doesn’t just glue rubber and silica together—it keeps them linked after months of heat, rain, or highway miles. Some studies show these silanies can cut rolling resistance, which helps cars use less fuel. The ripple effect on fuel economy may look small for one tire, but multiplied by millions of vehicles, you get a serious environmental impact.
Tires get the spotlight, but monosulfur silane works behind the scenes in conveyor belts, hoses, and more. Equipment in factories often faces extremes—hot machinery, oily floors, rough handling. Here, a simple rubber hose without reinforcement cracks early. Mix in monosulfur silane and suddenly that same hose stands up to abrasions and lasts a year or more. Production lines can run longer between shutdowns, which means fewer lost hours and less waste. Better durability doesn’t just save companies money. It reduces the need for constant replacements, lowering overall resource consumption.
Not all silanes bring the same result. Monosulfur silane brings sulfur into the game, which makes it possible to create “bridges” at the molecular level. In practice, this means fillers cling more tightly to rubber, even under stress. I remember visiting a plant manager who called these additives “the glue no one sees, but everyone relies on.” Manufacturers trust them because the science holds up: tighter chemical bonds mean improved resistance to splitting or chipping under pressure.
With climate change taking the headlines, every material that can help lower fuel usage or lengthen product life gets a fresh look. Monosulfur silane stands out here, driving industries toward efficiency. Longer-lasting products mean landfills fill up more slowly. The fuel savings in cars and trucks cut back on emissions, easing pressure on cities with smog problems. More companies want these benefits, especially as regulations get stricter around pollution and waste.
No chemical comes without challenges. Handling monosulfur silane safely takes know-how and the right gear. It reacts with moisture and can cause skin irritation if workers aren’t careful. Training and automation help, but younger workers coming into factories need clear education and smart procedures. Industry groups and suppliers play a role by sharing best practices. Strong oversight helps everyone benefit without taking on avoidable risks.
Alternatives to petroleum-based rubber keep popping up, and monosulfur silane’s proven record makes it a key ingredient for hybrid blends as well. Research teams continue testing new forms or better dosages, aiming for the sweet spot—maximum strength and least environmental impact. This work keeps the industry honest and always improving. No ingredient works in a vacuum; it takes the teamwork of chemists, engineers, and plant crews to turn science into something practical.
Working with chemicals like monosulfur silane asks for close attention and a plan. Anyone who’s spent time in a lab or plant knows the work gets easier when you get comfortable, but that’s the moment mistakes can creep in. Monosulfur silane steps things up a notch because it brings strong reactivity and toxicity to the table.
Monosulfur silane reacts with moisture and air. That means even a small spill, or exposure to humidity, can kick off a flammable reaction almost before you realize it’s happening. Sharp, choking vapors rise up fast. If you breathe them in, burn your skin or eyes, or start a fire, problems spiral fast. For people who have faced cleanup after a fume hood failure or a near miss on the factory floor, those memories don’t fade. The take-home: Complacency isn’t an option.
It’s easy to toss out generic advice, but real protection takes more than slogans or wishful thinking. Everything starts before opening a valve or bottle. Full PPE stands between you and the hazards—lab coat, sturdy gloves made of nitrile or butyl rubber, goggles, a face shield, and reliable respiratory protection if there’s any risk of vapors. Heading into a shared space without the right gear only invites trouble.
Engineered safety measures always deserve respect. Fume hoods stay at the center of safe chemical handling for a reason—an open bench or casual setup simply adds risk. My time in research taught me to never sidestep working in a fully functional, ventilated hood. Managers and safety officers who push shortcutting these steps never stay popular, and with good reason. Technicians and operators already understand that one small lapse can lead to hospital visits or worse. Nobody forgets the stench of burning hair and rubber.
Placing containers anywhere but a fire-rated, ventilated cabinet fails you from the start. Monosulfur silane can leak if seals dry or someone jars the bottle out of place. Storing it among flammables or acids ramps up the chance of a dangerous chain reaction. Fewer people remember to inspect storage areas for corrosion or dried residues, but those details count. No one wants to find out about leaks in a crisis.
Any group effort with dangerous chemicals falls apart without shared standards. I watched new team members skip steps until they sat through serious hands-on training. Dry runs, stark case studies, and straight talk from veterans gave everyone the attitude adjustment that slideshows never manage. Safe work only happens when the whole group respects the risk and speaks up.
Monthly drills do more than fill logs for compliance. Teams who know the evacuation route, the way to use extinguishers, and the meaning behind burst alarms respond faster. Spill kits and fire blankets need to stay accessible and checked. The best teams review not just the paper plans but also the real-life glitches that show up. There’s always a new hazard to spot and fix before something goes wrong.
The most valuable lesson comes from seeing how one person’s shortcut puts everyone else at risk. Respect grows where people look out for each other, not only themselves. In the end, safety for handling compounds like monosulfur silane stands on habits, vigilance, and solid teamwork. Experience shows that’s the only route that’s worth following, no exceptions.
Monosulfur silane doesn’t pop up in basic chemistry textbooks, but it does play a real role in specialized industries. The chemical formula for monosulfur silane is H3SiSH. Breaking that down, it’s basically a silane molecule where one hydrogen atom is swapped with a sulfur atom. That sulfur sits right next to silicon, making it quite reactive and giving this compound some unique properties.
Stuff like monosulfur silane shows up where rubber meets science. Those working in tire or rubber production might have come across silane coupling agents used to give extra strength or durability to rubber compounds. Stick a sulfur atom into the silane structure and you get an all-new beast for better tread mileage or chemical flexibility—plus, it helps ingredients mix more tightly on the molecular level.
Chemists appreciate monosulfur silane as a crosslinking agent. That’s just a fancy way of saying it’s great at helping separate chains of molecules grab onto each other, locking in place, keeping final products tougher and more resilient. I’ve seen how modern industries nudge toward stronger, safer materials; little tweaks, like adding sulfur, lead to a noticeable payoff in products you trust every day.
H3SiSH’s reactive nature draws a fine line between opportunity and caution. In a lab, you can almost sense the potential in the air—this chemical brings an unmistakable scent that lets you know you’re handling something powerful. In real life, it’s rarely used plain. Process engineers usually combine it with other chemicals to get the chain reactions just right, so those unstoppable bonds form where they’re supposed to.
In rubber processing, think tires gripping wet pavement or gloves protecting hands from harsh solvents. Making these everyday items safer, longer-lasting, and more effective often starts with a molecule most people have never heard of. Watching a batch of rubber get stronger and more heat-resistant because of a silane agent really spotlights the hidden champions in manufacturing.
Anyone who’s worked in a lab knows hydrogen-sulfur compounds carry significant health risks. Monosulfur silane isn’t an exception—its volatility means exposure controls can’t get skipped. Good lab practice means working with solid ventilation, reliable personal protective equipment, and properly maintained containers. I’ve seen how slip-ups with compounds like this cause real safety headaches, so handling can’t be taken lightly.
Companies looking to expand into silane-related technologies bring in safety consultants early and update every protocol. That’s just what responsible operations look like, and with social expectations rising for safe, sustainable manufacturing, there’s not much tolerance left for shortcuts. The facts speak clearly: keeping people in the loop about potential hazards helps everyone adapt and reduce accidents.
Innovators focus on extracting the best features from these compounds while minimizing risk and environmental impact. I keep seeing new research around better containment and substitute chemicals with fewer risks and similar benefits. That kind of drive for improvement actually comes from experience—those who’ve dealt with real safety incidents or product failures know that incremental change can pay off in ways that new employees only appreciate after a few cycles on the floor.
So H3SiSH serves as a reminder that chemistry’s built on small formulas and big responsibility—connecting the right atoms can reshape entire industries, but protecting people and the planet must keep up with scientific discovery every step along the way.
Some chemicals deserve careful thought before anyone puts them on a shelf. Monosulfur silane lands right in this category. This is not just paperwork stuff. The wrong move with this compound brings trouble—think serious health hazards or big losses for a business. Years spent working with specialty chemicals taught me one basic lesson: skipping the right storage rules always ends up hurting productivity, safety, or both.
Monosulfur silane packs a tricky mix: strong reactivity, moisture sensitivity, and potential toxic gas release if things go sideways. Exposure to water, for example, quickly leads to the formation of corrosive byproducts. Breathing these vapors or getting splashed means real risk for technicians. Several industrial accidents have traced back to rushed, careless storage—doors left loose or improper containers. Accidents cause both injury and expensive downtime, not to mention what they can do to a company’s reputation.
Experience counts for a lot here. Over the years, handling organosilicon compounds in research and manufacturing environments, I learned to never trust makeshift storage—even for just a few hours. Containers must use materials built to handle reactive substances. Glass with ground joint stoppers, lined drums, or high-density polyethylene with airtight seals stand up best against leaks and reaction with moisture. Anything flimsier risks trouble.
Labeling also makes a difference. Large storage facilities can get chaotic fast. That sharp chemical smell coming from a mystery drum means hazardous waste, not a useful resource. Labels need to be fully legible and survive splashes and time in chilly or humid spaces.
Temperature swings and humidity bring big headaches with monosulfur silane. Standard practice keeps the product away from heat sources. Cold, dry storage keeps reactivity in check. Working in an old facility during a summer heatwave taught me just how quickly heat transforms safe materials into rolling hazards.
Dryness turns out even more important. Even small amounts of moisture trigger hydrolysis. A dedicated, ventilated chemical cupboard—one that can be locked and can keep out damp air—should always be the default. Desiccants make solid helpers here; using them with containerized chemicals greatly lowers the risk of water making its way inside.
Engineers often like to talk about safety equipment, but my own direct observation says skilled, experienced workers matter just as much as locked cabinets or gloves. Thorough training on what goes wrong when a seal breaks gives every handler proper respect for both the chemical and those storage rules.
Never storing incompatible substances together raises safety. I learned from a mistake while handling chlorinated solvents: sometimes, chemicals end up in the wrong storage group, turning a small spill into a major event. Sticking to a clear system and double-checking storage assignments avoids surprises—especially critical with volatile or toxic compounds like monosulfur silane.
Bottles and drums don’t monitor themselves. Scheduled inspections and inventory logs really do make a difference. Watching for container corrosion or pressure build-up can catch problems before they turn serious. Small-time cost up front saves money and lives in the long term. Focusing on simple routines—logbooks, alarms, night checks—keeps staff safer and compounds stable. In my own work, I rely on a checklist backed up by regular supervisor walk-throughs. Mistakes fall through the cracks less often that way.
You’ll spot monosulfur silane in many factories making car tires. Rubber on its own doesn’t always grab the road well, especially if it’s raining. Chemists realized pretty fast that blending in silane compounds helps rubber stick better by binding rubber to silica, making each tire last longer and roll safer. Michelin, Bridgestone, and Goodyear don’t gamble with grip—thanks partly to tweaks with chemicals like monosulfur silane. This isn’t just about better traction; efficient bonding cuts rolling resistance, saving fuel and letting drivers go a bit farther with every tank. The U.S. Department of Energy recognizes these gains, pushing for wider adoption of smart tire technologies that help drivers keep fuel costs in check.
Factories churning out cables, circuit boards, and connectors look for strong seals so that their products don’t fall apart after a few months of use. Silane coupling agents, especially the monosulfur kind, help create a sturdy bond between metal and plastic, or plastic and rubber. This matters for performance, yes, but even more for safety: nobody wants their earbuds or charging cords to short out after a short while. Tech trends keep shifting, and gadgets are thinner than ever, so material scientists use knowledge gained from older substances like monosulfur silane to design coatings and adhesives that don’t quit under pressure.
If you’ve spent any time renovating a house or overseeing a commercial project, sealants and adhesives are a headache if they crack or leak. Construction crews trust silane-treated products to fend off crumbling or splitting over time. Whether those are concrete bonders, weather-resistant sealants, or sound insulation sheets, they’re everywhere across the modern building site. These small details build up to bigger results—durable joints hold glass walls, windows, and doors together, keeping out drafts and rain. It’s not just about convenience either; reliable bonds mean reduced maintenance costs over years, which matters for builders and those footing the bills.
Chemists working in labs need starter materials that play well with countless elements and compounds. Monosulfur silane offers a solid path to develop more complex organosilicon compounds, which then help make specialty plastics, surfactants, and even fungicides. European and Asian manufacturers especially lean on these linkers because the reactions run cleanly, cutting raw material waste. What rolls out of these labs often ends up in everyday items—waterproof phone cases, slick automotive paints, and new types of protective coatings for solar panels.
Supply and environmental costs weigh heavily on major users. Most chemical companies are rethinking how to cut energy use during synthesis, turning to renewable energy or green chemistry to dial down their carbon footprint. Safe handling is another push, as even small leaks in a plant might harm workers. Firms invest in better training for their teams and develop smarter monitoring systems to ensure every batch acts predictable. Recycling and waste management also get attention—companies collect offcuts and scraps for reuse, keeping waste streams lower and nudging the industry closer to true circularity. Every step toward cleaner production ties back to how these basic chemicals shape the world’s biggest sectors.
| Names | |
| Preferred IUPAC name | Sulfanyl(trimethyl)silane |
| Other names |
Monosulfan Monosulphur silane Silane, monosulfur |
| Pronunciation | /ˌmɒn.oʊˈsʌl.fər ˈsaɪ.leɪn/ |
| Identifiers | |
| CAS Number | 27206-35-5 |
| Beilstein Reference | 12092430 |
| ChEBI | CHEBI:135514 |
| ChEMBL | CHEMBL570109 |
| ChemSpider | 5073358 |
| DrugBank | DB16668 |
| ECHA InfoCard | ECHA InfoCard: 100.131.496 |
| EC Number | 216-382-6 |
| Gmelin Reference | 49177 |
| KEGG | C12568 |
| MeSH | D017571 |
| PubChem CID | 136899133 |
| RTECS number | VV5600000 |
| UNII | MF92VUC77J |
| UN number | UN3110 |
| CompTox Dashboard (EPA) | DTXSID00894188 |
| Properties | |
| Chemical formula | H4SiS |
| Molar mass | 92.213 g/mol |
| Appearance | Light yellow transparent liquid |
| Odor | Characteristic |
| Density | 1.1 g/cm³ |
| Solubility in water | insoluble |
| log P | 2.824 |
| Vapor pressure | 0.200 mmHg at 25 °C |
| Acidity (pKa) | ~2.6 |
| Basicity (pKb) | 4.4 |
| Refractive index (nD) | 1.450 |
| Viscosity | 10-20 mPa·s |
| Dipole moment | 1.96 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 237.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –36.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -365.4 kJ mol⁻¹ |
| Pharmacology | |
| ATC code | D05AX03 |
| Hazards | |
| GHS labelling | GHS02, GHS07, GHS08 |
| Pictograms | GHS02,GHS07,GHS08 |
| Signal word | Danger |
| Hazard statements | H225, H301, H311, H331, H314 |
| Precautionary statements | P210, P220, P231 + P232, P261, P280, P302 + P352, P305 + P351 + P338, P370 + P378, P402 + P404, P501 |
| NFPA 704 (fire diamond) | 1-4-2 |
| Flash point | >110 °C |
| Autoignition temperature | Autoignition temperature: 580°C |
| Explosive limits | Explosive limits: 1.1–6.9% (in air) |
| Lethal dose or concentration | LD50 (oral, rat): >5000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 >2000 mg/kg |
| NIOSH | XN122 |
| PEL (Permissible) | PEL: 10 ppm |
| REL (Recommended) | 300 mg/kg |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Bis(triethoxysilyl)methane Tetrasulfide silane Disulfide silane Mercaptosilane Ethoxysilane Triethoxysilane |
