Chemists didn’t simply stumble across Ditert-Butyl(Trifluoromethylsulfonyloxy)Silyl Trifluoromethanesulfonate—often referenced in research circles under various shorthand names—by accident. This compound came out of the ongoing search for silylating agents that push boundaries in selectivity and stability. Back in the late 20th century, organosilicon chemistry needed tools that worked reliably for complex syntheses, especially for protecting groups on sensitive alcohols and phenols, and so labs tuned the structure of silylating reagents. Researchers drew on both theory and trial-and-error, following up on hints from trifluoromethanesulfonate (triflate) chemistry, and ultimately produced these robust reagents. In my own lab experience, the step from classic TMS (trimethylsilyl) reagents to something as nuanced and effective as a ditert-butyltriflate silyl reagent reflected the maturity of silicon chemistry as a discipline. Now, many research groups rely on the fine balance of sterics and electron-donating effects offered by such compounds to solve new problems in molecular construction.
Ditert-Butyl(Trifluoromethylsulfonyloxy)Silyl Trifluoromethanesulfonate attracts attention for the unique way it balances bulk and reactivity. The molecule carries both ditert-butyl and trifluoromethanesulfonate groups, making it much more than a niche compound. This chemical lands in the toolkit of synthetic and medicinal chemists looking for efficient silylation and functional group transformations. The product usually comes as a colorless to pale yellow liquid, resistant to water and packed under inert gas to avoid degradation. Commercial suppliers generally offer it in amber glass bottles, specifically for research and development labs, and not for direct therapeutic or household use. My own order came with a tightly sealed flask, reinforced by chilling packs, and clear warnings that hinted at how energetic and unforgiving these chemicals can be in the wrong hands.
This silyl triflate owns a distinct chemical fingerprint. The presence of ditert-butyl groups gives bulk and shields the silicon atom, while the trifluoromethylsulfonyloxy group acts as a powerful leaving group, making the molecule highly reactive in silylation reactions. As a liquid with a moderate boiling point and low volatility, it proves easier to handle in a glove box than many air-sensitive reagents. In practice, its reactivity rivals that of the best silylating agents available. You get a sharp, acrid odor on accidental exposure, which adds an extra reminder to always work under proper ventilation. Both the density and miscibility with common organic solvents make it easy to use in batch syntheses, yet its strong Lewis acidity and electrophilicity mean even trace moisture or nucleophiles can trigger unpredictable decomposition. Everything I've learned about handling aggressive reagents still holds true—one slip, and the results can be disastrous both for your reaction and your safety.
Any legit chemical comes with a detailed safety data sheet and technical bulletin. For Ditert-Butyl(Trifluoromethylsulfonyloxy)Silyl Trifluoromethanesulfonate, commercial sources list purity (typically above 97%), density, and a CAS number for reference. Specifications clarify storage below 4°C, away from light and moisture. Clear hazard identification appears on every bottle: corrosive, harmful if inhaled, and capable of causing burns on contact. From personal experience, missing a glove or having an old, cracked stopper just isn’t worth the risk. The product arrives labeled for laboratory use only, not for food, drug, or cosmetic applications. Batch certificates also describe spectral characteristics (especially NMR and IR absorption peaks), ensuring synthetic chemists get exactly what the protocol demands.
The route to Ditert-Butyl(Trifluoromethylsulfonyloxy)Silyl Trifluoromethanesulfonate starts with rigorous exclusion of water and oxygen. Typically, a ditert-butylchlorosilane precursor reacts with trifluoromethanesulfonic acid or its anhydride under anhydrous conditions. The triflate group replaces the chloride, sometimes aided by a tertiary amine base to absorb HCl evolved during the procedure. Industrial-scale synthesis uses large Schlenk lines, distillation, and scrupulous purification by column chromatography, but smaller labs usually work in gloveboxes or under dry nitrogen to avoid nasty surprises from hydrolysis. I’ve seen skips in the purification step leave behind colored impurities, which mess up downstream reactions and waste valuable material. Only through trial, patience, and strict method following does the pure liquid emerge, ready for use or careful bottling.
This reagent gains most of its value in silylation—introducing protective silyl groups onto alcohols, amines, and sometimes acidic protons on heterocycles. The ditert-butyl silyl group is large, so it blocks more than just the most accessible reaction sites. I’ve used this in complex molecule synthesis to select specific hydroxyls for protection while leaving others untouched. The triflate leaving group reacts fast, meaning reactions often finish in minutes under mild conditions. After silylation, the resulting silyl ethers stand up to acids and bases better than those derived from smaller silyl groups, which lets chemists perform more aggressive transformations before removal. Some papers discuss mild fluoride-based deprotection, and I’ve seen teams patent proprietary protocols to recover or switch out these groups at later synthetic stages. From my own bench work, the main hitch comes if too much reagent is used—side reactions and cost waste can balloon quickly.
In catalogs and literature, you may see the chemical listed under names like Ditert-butylsilyl triflate, TBSOTf, or bis-tert-butylsilyl trifluoromethanesulfonate. Each name arises from a different context—some focus on the silyl group, others on its powerful triflate leaving group. Having sorted through supplier lists myself, those multiple entries can confuse a newcomer, especially given synonyms overlap with different yet related silylating agents. Always double-check CAS and structural diagrams before ordering; nothing ruins a week like trying to troubleshoot reactions with the wrong chemical on hand.
Direct experience made me respect the danger these sulfonyloxy silyl reagents pose. Quick skin contact leads to burns. Inhalation isn’t just an irritant; it can cause long-term respiratory issues, so working in a certified fume hood, with gloves and goggles, is the only acceptable practice. Strict storage under argon or nitrogen prevents hydrolysis and dangerous decompositions. Any spilled liquid gets neutralized with sodium bicarbonate solution and wiped with copious water, but only after removing solvents that react vigorously. Training lab techs and students on these risks isn’t optional—neglected standards can escalate to hazardous incidents, halted projects, and regulatory headaches. Waste disposal must travel through a container marked for silicon- and sulfur-containing organics, destined for incineration at specialized facilities.
Synthesis of complex molecules—ones decorated with multiple reactive groups—depends on reliable protective groups. Ditert-Butyl(Trifluoromethylsulfonyloxy)Silyl Trifluoromethanesulfonate supports this in academic and pharmaceutical labs, especially in assembling oligosaccharides, peptides, and natural products. My project on glycosylation benefited tremendously from this reagent’s selectivity; the silyl group protected a stubborn hydroxyl that otherwise derailed coupling steps. Medchem labs use these silyl ethers to stage-lay synthesis without wasting time on failed routes. Even agrochemical research and advanced material science leverage ditert-butyl silyl ethers for making functional polymers and hydrophobic coatings. Process chemists keep an eye on cost and scalability, but for small-volume high-value targets, this reagent justifies itself through saved effort and higher overall yield.
Research attention centers on tuning reactivity, selectivity, and deprotection strategies associated with these silyl triflates. Some groups work on milder, “greener” preparation routes, aiming to cut down on hazardous byproducts or lower the expense of precursor materials. Studies compare different silicon frameworks to see which combinations give the sharpest discrimination between similar alcohols. Teams regularly publish modifications and strategies to streamline downstream removal, since complex molecule synthesis lives or dies by reagent compatibility. Last year, I read a series of articles showing that next-gen silylating agents, tailored for stereospecific reactions or enzyme compatibility, started from the lessons learned by working with ditert-butyl triflate silyl chemistry. Chemistry societies continue to sponsor grants and symposia dedicated to organosilicon research, ensuring that the pace of discovery doesn’t let up as new materials and medicines demand ever smoother synthesis.
Animal studies and in vitro assays paint a clear picture—prolonged or intense exposure leads to chemical burns, tissue necrosis, and delayed organ damage. While single-use exposures, managed with good ventilation and PPE, present low chronic risk, accidental spills or inhalations cause acute symptoms. Most labs enforce spill protocol drills and medical monitoring when working with any strong electrophile like silyl triflate derivatives. Environmental impact, particularly on aquatic organisms, requires responsible handling and destruction of waste; silyl triflates persist and disrupt biological activity in runoff. Regulatory bodies have started ramping up label warnings and reporting standards for silicon sulfones, raising the compliance bar for both shipment and disposal. Speaking from personal experience, I’ve seen research groups lose grant funding after violating disposal policies, which means tighter compliance benefits both health and funding security.
Trends in molecular design and sustainable chemistry keep driving interest in silylating agents that act faster, with less toxic waste, on a growing menu of target molecules. As molecular engineering leans into chiral, sterically congested frameworks, reagents like Ditert-Butyl(Trifluoromethylsulfonyloxy)Silyl Trifluoromethanesulfonate will keep evolving. Teams search for catalyst systems or greener solvents compatible with these agents, and some startups are beta-testing cartridges meant for on-demand reagent generation, so research groups don't have to store large, hazardous stashes. Increased automation and in-line analytical monitoring already help spot mistakes before they ruin high-value syntheses. In my view, chemists who keep sharpening their understanding of organosilicon compounds, and adopt a rigorous approach to safety and innovation, will stay at the front of the next wave of discoveries, creating molecules that today’s techniques can only dream of building.
Chemistry often revolves around finding just the right tool to build or tweak a molecule. Ditert-butyl(trifluoromethylsulfonyloxy)silyl trifluoromethanesulfonate may turn up a mouthful on the label, but among synthetic chemists, it offers a mix of power and precision. I’ve watched reactions stall or meander until swapping in a genuinely effective silylating agent—this particular compound often gets praise in those moments.
In the world of organic chemistry, silylating agents protect sensitive groups and help move projects toward more complex targets. This reagent steps into the game when folks need to attach tert-butyldimethylsilyl (TBDMS) groups efficiently. Classic silyl chloride approaches can hit obstacles: tricky side reactions, moisture sensitivity, tough conditions. With ditert-butyl(trifluoromethylsulfonyloxy)silyl triflate, the process gets much cleaner. The compound’s high reactivity means silyl ethers of alcohols or phenols form easily, even at low temperatures and without harsh bases. Synthetic teams sometimes joke that this is the shortcut you wish you found during grad school—no sticky columns or mystery side products.
Speed matters, especially in multi-step total syntheses. A slow or unpredictable silylation could drag a process down for days. This compound works with stubborn substrates like hindered alcohols and works fast enough to keep a project on schedule. A friend of mine once used it to protect a tertiary alcohol right in the final step of a tricky route—you save time, you get better yields, and you dodge the headaches tied up with older reagents.
Selectivity comes up again and again in lab stories with this tool. In cases where plain silyl chlorides scatter their efforts or need heavy-handed conditions, this reagent keeps things straightforward. Chemists juggling multiple reactive groups need a silylating agent that knows where to stop, where to act—this silicon-based tool just gets it right more often than not.
Carbohydrate chemistry relies on well-paced protection and deprotection steps. Getting selective silylation on a single hydroxyl group out of a crowd can mean the difference between isolating a prized product or sorting through a tangle of side reactions. This reagent gives researchers the upper hand, letting them dial in the right structure. In my own attempts to build up carbohydrates, I saw that the difference between a crisp yield and a sticky mess often came down to these selective moves.
Nucleoside chemists tell similar stories. Tweaking the sugar ring without disturbing the nucleobase or other sensitive groups demands finesse. This silylating agent stabilizes intermediates without dragging along impurities, giving cleaner results in key steps of antiviral or anticancer work. Even peptide chemists are jumping in—fewer side reactions make for purer final products.
While new reagents light up labs with their efficiency, there’s always the question of safety, waste, and scalability. Triflate reagents carry a reputation for high reactivity—great when you want a clean reaction, but they need real respect at the bench. I’ve seen teams invest in better ventilation and handling protocols. Using this compound saves time and reduces chemical waste downstream because you skip repeated purifications and minimize failed reactions.
Chemistry always pushes for solutions that fit current demands while leaving the door open for safer, greener options. This reagent fills gaps in efficiency and selectivity, but every lab analyst who’s handled it has kept one eye on safer, more sustainable alternatives. Until a perfect replacement shows up, ditert-butyl(trifluoromethylsulfonyloxy)silyl triflate holds its place as a favorite for the jobs where reliability and results count.
Safe storage helps protect health, business, and the environment. I’ve worked in a laboratory where one spilled bottle of a solvent turned a standard afternoon into a hazardous mess. That day, we all learned fast that a little attention to storage saves a lot of trouble. Chemical products can easily cause harm when not handled carefully. This is why clear conditions, updated data sheets, and attention to detail really do pay off.
A typical storeroom runs at about 20 to 25°C, out of direct sunlight, and away from heaters or freezing drafts. These conditions fit basic household cleaning agents, yet plenty of specialized chemicals react badly when stored like this. Acidic or basic solutions may corrode metal shelving; solvents might slowly eat through plastic containers. If humidity creeps up or the room stays closed and steamy, powders may clump, cakes can form, or containers start to bulge as pressure builds up inside.
Light-sensitive substances degrade when exposed, so I’ve learned to use amber bottles for these products. Heat speeds up reactions and creates pressure. I once saw ammonium nitrate containers start sweating on a hot day; we hustled them into a cool storage locker out of concern for safety. Moisture invites mildew and encourages chemical breakdown. Keeping desiccants inside storage cabinets helps, and it’s smart to check those little packets now and then—they do become saturated over time.
Labels do more than show which product sits on the shelf. They remind anyone in the room of flammability risks, poison hazards, or safe handling instructions. Poor storage practices show up in regular news stories about businesses or schools facing expensive cleanups. Keeping acids away from bases, flammables in a dedicated cabinet, and incompatible materials on different shelves cuts down the chance of unexpected reactions. Locking up high-risk chemicals prevents tampering and reduces liability.
Trusted sources like the Safety Data Sheet (SDS) walk users through safe storage, including temperature range, ideal container type, and what to avoid stacking nearby. Industry professionals rely on OSHA and NFPA guidelines for a reason—they’re backed by years of experience and research. As a technician, I once found out the hard way that skipping a line on a safety sheet could mean a surprise inspection or worse. Reading and following guidelines saves headaches and keeps operations running smoothly.
Before opening any new chemical, look for the SDS and scan the critical sections about storage. Inspect containers for cracks or signs of wear. Shelving should support all weight and allow for spacing between bottles. Spills happen fast; keeping absorbent pads and neutralizers close by helps keep damage under control. Regular reviews of stock prevent expired chemicals from building up and reduce surprises during audits. In my own workspace, a tidy, well-labeled shelf builds confidence not only for safety but also for consistent results in every experiment or process.
Smart chemical storage goes beyond regulations; it brings confidence to daily work and keeps communities safe. Neighbors don’t want risk nearby, and employees deserve an environment where they can work without fear. Companies lose reputation and revenue over poor storage events, while families face health risks if even small quantities of strong chemicals get mishandled at home. Small investments in training, storage units, and routine checks help everyone sleep easier at night.
Long, technical names sometimes hide huge risks. This chemical pulls double duty: it’s a strong silylating agent and also packs the reactive punch of two different triflate groups. As a tool in organic synthesis, it opens doors to reactions fast and clean. Yet, that efficiency runs parallel to real hazards: corrosivity eats at skin and eyes, strong fumes sting the lungs, and reactivity loves to turn violent if careless hands come near. In my years working with organosilicon materials, the fastest mistakes usually appeared during transfers and cleanup, when familiarity breeds shortcuts.
Organic chemists joke about “Hazmat chic” but there’s no glamour scrubbing burns from hydrolysis accidents off arms. Splash goggles and a heavy face shield block nasty eye injuries. Nitrile gloves double-layered, real lab coats snapped tight, and chemical-resistant sleeves set up an armor everyone grows to trust. I watched a colleague ignore a stubborn bottle cap, grab it barehanded, and land in urgent care. One rushed second, three months recovering.
Organic volatiles love finding ways into the air. This compound gives off acidic vapors that stick to membranes inside the lungs. Keeping experiments locked inside certified fume hoods feels obvious—until the HVAC system fails. You notice right away: tickle at the nostrils, eyes start to burn, voice sounds hoarse. I‘ve seen too many labs shut down for days after a single spill, air scrubbers blasting on overtime. Close those sashes, use proper ducting, and treat every transfer as a contained operation.
No one ever learned safe handling by guesswork. The most effective workgroups have lived every “worst-case” drill. Spills get treated as emergencies, not minor annoyances. Neutralizers like sodium bicarbonate sit loaded and ready. Wash stations and eye baths aren’t afterthoughts—they’re at every exit. Safety data sheets get more than a glance, and every new team member runs tabletop exercises before their first solo day. Once, we held a five-minute safety chat before every shift, and accident counts dropped in half that quarter.
This chemical reacts fast with trace moisture. Seals dry and tight make the difference between weeks of steady use and discovering a wrecked batch of brown sludge two mornings later. Silica packs multiplied along shelves, solvent bottles stacked on bottom, and no flammable acids anywhere within reach. Old school heat detectors and standard refrigerators won’t cut it—temperature swings mean volatility climbs fast. I keep a logbook for every bottle, old school but it works: use oldest first, check for pressure bumps, record any sign of leaks.
Waste disposal walks a tightrope. Pouring left-over material down the sink just isn’t an option. Even tiny drips can start local corrosion inside pipes or gas off acidic fumes that linger long after the lab has emptied for the day. Secure containers, chemical-resistant liners, and certified waste contractors take the guesswork out. Nobody remembers all the rules offhand, but a quick sign on the wall with steps and contacts keeps mistakes rare. Last year, a single unmarked bottle landed a team in a drawn-out regulatory audit.
Staying alive isn’t complicated: tight habits, constant practice, and the humility to ask for help every time something seems off. There’s nothing macho about chemical burns or hospital visits. Facilities that invest in training, ventilation, and community foster teams that work safer, smarter, and longer. Speaking from experience—confidence comes from tight systems, not shortcuts.
Every time I look at a new compound, the first thing that comes to my mind is: how does its structure shape what it can do? Chemistry teachers always said that shape tells the story, and they were right. The bonds between atoms, whether tight or loose, matter a lot for almost everything: boiling, melting, dissolving, or even reacting with your skin if you spill it. Shapes decide how molecules stack up, how electrons travel, and how stable the stuff really is. Everyone who works in a lab gets that weird buzz before running a simple melting point test—waiting to see a number they can trust. Melting and boiling points, solubility, color, texture—these are a chemist’s first steps in getting to know a new chemical.
When I first handled samples years ago, I learned quickly not to take appearances for granted. Sometimes a crystal shines bright but smells harsh; sometimes a perfectly clear liquid turns out to be dangerous. So many physical properties jump out right away: color, density, hardness, taste (though honestly, nobody in the lab tastes anything, despite what textbooks claim), and odor. Texture under the spatula makes a difference. Powders flow or clump. Granules stick or bounce around. Liquids might run like water or sluggishly drip, slippery and dense.
Water solubility still rules most industries. If it dissolves easy, it travels through pipes, moves in the body, or mixes into almost anything. Density can separate heavy stuff from the rest, and that matters for storage, transport, or disposal. The melting point tells you if it will survive a hot summer or spill out on a cold morning. Chemists learn early that these simple facts shape the risks and opportunities of any material. In one memorable project, a compound with an odd melting point forced the team to rethink every part of the handling process.
Reactivity sits at the core of chemical properties. Will it catch fire, corrode metal, or simply ignore everything else? Flammability, acidity, basicity—each trait hints at a set of risks and benefits. Labs and factories both want to know: Will this compound break down in air? Will it foam when mixed with acids or stay silent? One strong acid spilled on a floor at my first internship. Everyone remembered the lesson: chemical properties can shape safety protocols and reputation overnight.
Sometimes, the structure gives clues. Rings of carbon, noisy groups like nitro or amino, or simple chains—they all tell a story. Organic compounds find uses in medicine, plastics, food, and more because they react and join together easily. Inorganic compounds, steadier or quicker to lose electrons, clean water, brighten colors, build batteries, and treat soil. Oxidizers need special storage, and anything with strong acids gets double checks for seals and gaskets. Toxicity matters too: is it safe on the skin, or does it need gloves and a vented hood? Regulations come down to questions like that.
Good data on compounds, always shared with clear instructions, powers safety and innovation. Training people to understand melting points, flammability, and solubility cuts down on mistakes and keeps everyone out of trouble. Replacing hazardous chemicals with less toxic cousins or swapping out something unstable for a robust substitute makes work and life safer. Green chemistry, with its push for non-toxic and biodegradable options, keeps pushing boundaries. Every small step—better labeling, smarter storage, quicker communication—moves things forward for everyone working with chemicals. Years in labs taught me to never underestimate the basics; physical and chemical properties steer the entire journey, from the beaker to the big world outside the lab.
Nobody enjoys flipping through page after page of warning labels, but safety information isn't just corporate fine print. Incidents with widely-used products show how easily things can go sideways if we skip the details. Over time, even seemingly harmless purchases have caused real trouble—think of products that trigger allergic reactions, or cleaning chemicals that cause headaches and hospital visits.
Looking back, I once mixed a “natural cleaner” with something stronger inside a cramped bathroom. The air thickened, skin tingled, and a few minutes later, my throat started burning. I learned quickly—chemical combinations deserve more respect than we sometimes give. These kinds of mistakes are surprisingly common. Consumer Product Safety Commission (CPSC) consistently reports thousands of injuries each year from items like cleaning sprays, batteries, and children’s toys. Many result from incorrect storage or misunderstanding what shouldn’t be mixed or combined.
Not every hazard jumps out at you. Sometimes it’s a slow, quiet process: lead paints flake off old window sills, cleaners release toxic fumes in closed spaces, lithium-ion batteries overheat if crushed or exposed to water. These risks don’t just pop up in laboratories––they show up in kitchens, garages, and pockets. News stories in recent years highlight children injured by swallowing button batteries, hand sanitizers causing skin burns, and fires started by cheap electronics. In much of this, the information was there, tucked away somewhere in small print.
People often trust familiar brands or rely on habits learned from family. “I’ve always done it this way, nothing’s happened before.” It’s only when things go wrong that we start asking, “Could I have known this in advance?” Chemical compatibility falls into this trap—mixing ammonia and bleach has always been risky, but many don’t know it creates poisonous gas. Sometimes incompatibility isn’t chemical. Wire a lamp with the wrong type of bulb, try charging a phone using a knock-off cable, or let a strong magnet near your solid-state drive, and you may lose more than expected.
People who want to make safer choices can arm themselves with better information. Government databases, like those run by the FDA, EPA, or OSHA, share product recalls, injury reports, and compatibility warnings. Don’t just scan for the green check mark; take a minute to check if this item is known to interact badly with everyday household things. For example, even soaps and lotions sometimes react with prescription drugs. Not all hazards can be seen or smelled.
Companies have a responsibility here too. No one wants fine print hidden behind complex language. Clear hazard statements, obvious icons, and honest reporting of accident histories help people trust that a product does what it says—and doesn’t hide risks. In my own circle, we learned to look closer after a friend’s toddler ended up in an ER from a detergent pod. Now we keep cleaning agents high up, old power strips out of reach, and labels visible.
The biggest step is to slow down, read just a little closer, and ask questions. Did this ever hurt someone? Does it work safely with stuff I already have? Most hazards aren’t new, but they’re easy to forget. Building habits around these questions pays back every time we avoid the ER or spare ourselves the stress of a household accident.
![[Ditert-Butyl(Trifluoromethylsulfonyloxy)Silyl] Trifluoromethanesulfonate](/static/81c4c90b-3bfe-4770-bbec-fcbf5e0a3809/images/2d/ditert-butyl-trifluoromethylsulfonyloxy-silyl-trifluoromethanesulfonate.png)
![[Ditert-Butyl(Trifluoromethylsulfonyloxy)Silyl] Trifluoromethanesulfonate](/static/81c4c90b-3bfe-4770-bbec-fcbf5e0a3809/images/3d/ditert-butyl-trifluoromethylsulfonyloxy-silyl-trifluoromethanesulfonate.gif)
| Names | |
| Preferred IUPAC name | bis(2-methylpropan-2-yl)-[trifluoromethyl(oxido)λ⁶-sulfanyl]oxy-trifluoromethanesulfonium |
| Other names |
Di-tert-butylsilyl trifluoromethanesulfonate DTBS triflate Di-tert-butylsilyl triflate Di-tert-butyl(Trifluoromethylsulfonyloxy)silane trifluoromethanesulfonate |
| Pronunciation | /daɪ-ˈtɜːrt-ˈbjuːtl ˌtraɪˌflʊəroʊˌmɛθəlˌsʌlˈfɒnɪˌɒksi ˈsɪliːl ˌtraɪˌflʊəroʊˌmɛθeɪnˈsʌl.fəˌneɪt/ |
| Identifiers | |
| CAS Number | 191603-80-4 |
| 3D model (JSmol) | `C[Si](C)(C)(C)OS(=O)(=O)C(F)(F)F.OS(=O)(=O)C(F)(F)F` |
| Beilstein Reference | 1868736 |
| ChEBI | CHEBI:139059 |
| ChEMBL | CHEMBL4294853 |
| ChemSpider | 33118021 |
| DrugBank | DB08286 |
| ECHA InfoCard | 100.264.224 |
| EC Number | This compound does not have an assigned EC Number. |
| Gmelin Reference | 1275050 |
| KEGG | C18367 |
| MeSH | C09K 53/10 |
| PubChem CID | 139405844 |
| RTECS number | WN6807000 |
| UNII | 53U55Q8U6V |
| UN number | 3272 |
| Properties | |
| Chemical formula | C13H22F6O6S2Si |
| Molar mass | 510.41 g/mol |
| Appearance | White to off-white solid |
| Density | 1.67 g/cm3 |
| Solubility in water | Insoluble |
| log P | 2.9 |
| Acidity (pKa) | -4.3 |
| Basicity (pKb) | pKb: -13.11 |
| Magnetic susceptibility (χ) | −83.0×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.322 |
| Dipole moment | 4.8857 Debye |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 554.8 J·mol⁻¹·K⁻¹ |
| Hazards | |
| Main hazards | Harmful if swallowed, causes skin irritation, causes serious eye irritation, may cause respiratory irritation. |
| GHS labelling | GHS02, GHS07, GHS08 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H314: Causes severe skin burns and eye damage. |
| Precautionary statements | P210, P261, P273, P280, P305+P351+P338, P310 |
| NFPA 704 (fire diamond) | 1-0-2-W |
| Flash point | Flash point: 113 °C |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.5 mg/m3 |
| Related compounds | |
| Related compounds |
Trimethyl(trifluoromethanesulfonyloxy)silane Triethyl(trifluoromethanesulfonyloxy)silane Tert-butyldimethyl(trifluoromethanesulfonyloxy)silane Trifluoromethanesulfonic anhydride Trimethylsilyl trifluoromethanesulfonate |
