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Chemistry has a rich tradition of inventing tools to move both science and industry forward, and 1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane bis(tetrafluoroborate)—sometimes called Selectfluor—proves how right compound at the right time shapes an entire field. Researchers in the later decades of the last century, driven by the limits of old-school electrophilic fluorination reagents, found themselves needing something with both brute force and finessed selectivity, but none of the risks that made many chemists nervous to use fluorine sources in the first place. The arrival of this reagent didn’t just answer that call; it shifted the dialogue. Its introduction bridged the gap between harnessing the impact of electrophilic fluorine with less reliance on barely-tamable sources like F2 gas or toxic compounds such as hypofluorites, which in practice were more likely to blow up than to serve as a reliable lab benchtop tool. In research labs, the arrival of this salt coincided with a boom in medicinal, agrochemical, and material science chemistry. Chemists could do things with fluorine that were never practical before: install it on rings, pipes, chains—wherever selective oxidation or fluorination was previously hamstrung by technical issues or the baggage of hazardous reagents. That story is more than just a tale of new molecules; it’s about progress that spilled over into commercial pharmaceuticals, agrochemicals, and polymer applications. Whenever visiting major synthesis conferences nowadays, the impact of this compound—sometimes called F-TEDA-BF4—is hard to overlook.
1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane bis(tetrafluoroborate) stands out because it’s stable on an open shelf, usually for months, comes as a fine crystalline white solid, and doesn’t require a fortification of special hoods or elaborate safety gadgets to handle on a reasonable scale. Chemists like its balance: aggressive enough to fluorinate fairly stubborn carbon centers while skipping the drama that other fluorinating agents bring. The structure itself is no accident—its quaternary ammonium backbone houses both the chloromethyl and fluoro components in a tight, caged configuration, stabilized by a pair of tetrafluoroborate counterions. This set-up makes it a true “bench-top” source of electrophilic fluorine, which cannot be said for most of its predecessors. With a melting point well above room temperature, the salt resists decomposition under most lab conditions, meaning less worrying about short shelf lives. Its reasonable solubility in common organic solvents like acetonitrile streamlines method development for organic synthesis in both academic and industrial settings.
The physical properties may read dry on a safety sheet, but in day-to-day chemistry, they explain why this compound dominates its niche. The solid spills easily into vials and weighs precisely on a balance, unlike hazardous gaseous alternatives, making its use far less intimidating for lab techs and junior researchers. The compound promotes reactions at room temperature—a huge win for any chemist interested in eco-friendly or “green” chemistry tactics, since high-temperature requirements drain energy and cost. Its shelf stability translates directly into reduced waste and lower operational risk: labs can keep a bottle handy for months, not days, which speeds up project timelines and slashes hazardous material expenses.
Every bottle of this compound comes with well-documented purity, water content, and batch-specific trace impurity data, fulfilling the string of regulatory and laboratory requirements for traceability. Such transparency backs up the quality claims that make its consistent use possible in validated processes. Scientists rely on these standards not only for laboratory reproducibility but also for scaling syntheses straight into pilot plant runs or industrial campaigns. Handling guidelines offer direct warnings for the seasoned chemist: eye and skin protection, minimal inhalation, and strong ventilation go from being optional extras to necessary steps, because the compound may irritate or react with residual water or nucleophilic species if handled carelessly.
Interest grows not just from the compound's end-use, but also from the reliability and accessibility of its synthesis. Year after year, literature highlights routes that generate high yields and proper quality without laborious, cost-prohibitive steps. Its preparation runs through methylation and fluorination steps applied to 1,4-diazabicyclo[2.2.2]octane—popularly called DABCO—followed by isolation and purification as the bis(tetrafluoroborate) salt. These methods don’t require specialty equipment and stay within the reach of most academic and industrial outfits. Scale-up doesn’t bring new hidden risks, a detail that sped up commercialization and routine application in research facilities.
Selectfluor and its relatives open doors in organic chemistry simply by behaving in ways that other agents cannot. Its “grab-and-deliver” style of fluorine transfer gives consistent results across a range of substrates, including those with aromatic rings, activated methylene groups, or complex heterocycles. The reagent shines in late-stage functionalization, particularly in pharmaceutical discovery. Adding a single fluorine atom can radically improve a drug’s metabolic stability or change its binding to a protein target, and Selectfluor’s predictable chemistry earns it a top spot in medicinal chemistry playbooks. Chemical modifications of the TEDA cation or pairing with different counterions extend the toolkit even further, allowing scientists to tune solubility, reactivity, or selectivity.
Walk through the hallways of any synthetic chemistry department, and this compound gets called by a half-dozen names: Selectfluor, F-TEDA-BF4, 1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane bis(tetrafluoroborate), or even just “that fluorinating salt.” Literature from the early 1990s onward overflows with these synonyms, making cross-checking research results a job for only the careful. Each alias reflects a phase in its adoption: from obscure research compound to staple in high-throughput medicinal chemistry.
The push-pull between performance and safety defines lab culture, and this fluorinating salt walks a fine line. It steers clear of the explosiveness and acute toxicity records of some other lab fluorine sources, but no one welcomes direct skin or eye contact, or high-level inhalation. Labs require gloves, goggles, and reasonable airflow to minimize chronic exposure, and waste disposal calls for more than a quick toss into aqueous waste or municipal trash. EHS teams rightly train staff to treat this as a moderate-hazard oxidant, which means routine risk assessments stay part of the workflow. For those managing research facilities, the safety track record of Selectfluor-type compounds means reduced insurance costs and peace of mind, especially compared to legacy fluorine chemicals that can turn a spill into a building-wide emergency.
This compound first made waves in the corridors of pharmaceutical chemistry, where selective fluorination sets apart blockbusters from also-rans. Its broad substrate scope let chemists fine-tune leads, adjust metabolic profiles, and increase the potency or longevity of new medicines. The tool isn’t just for pharmaceuticals. Agrochemical research uses it to build more weather-stable or bioactive pesticides and herbicides, making crops tougher and harvests more reliable. Polymers and material sciences also reap the reward: for electronics, new superacids, or thermal coatings, having a reagent like this allows incremental property improvements that add up to better batteries and more durable plastics. In academic research, Selectfluor reactions often feature in advanced organic synthesis courses, training new scientists for the challenges of applied fluorine chemistry.
With growing adoption comes real scrutiny on environmental and health impacts. Toxicology reports for 1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane bis(tetrafluoroborate) show moderate irritancy, calling for protective handling, yet mark it safer than older fluorine sources notorious for severe acute health hazards. Research articles from regulatory science journals point to rapid hydrolysis in aqueous media, which limits its persistence in the broader environment, but persistent monitoring forms part of “best practice” for all labs working with fluorinated compounds. Academic and industry toxicologists keep hunting for potential chronic effects stemming from long-term exposure, and so far, the compound maintains a clean enough record to justify continued use. Nonetheless, I’ve seen researchers argue for even greener, less hazardous fluorinating agents to keep up the drive toward sustainable chemistry.
In my career, watching new tools edge into the lab and stay in rotation means they do more than simply get the job done; they address both the demands of efficiency and growing concerns about health and ecological footprint. Efforts to engineer next-generation fluorinating reagents look to improve not just reactivity or selectivity, but to push toward fully renewable raw materials, safer breakdown products, and streamlined waste disposal. The competitive push comes from both regulation and smart consumers who demand safer, greener chemicals in the finished products they use every day. The story of Selectfluor and compounds like it suggests something important: chemistry does not stall out or stagnate. Instead, solutions born out of frustration with the old ways inspire generations of innovations making science both more productive and safer for all stakeholders.
In every lab I’ve worked in, the toolbox of reagents usually includes a few odd-shaped bottles with complicated names. 1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane bis(tetrafluoroborate), often called Selectfluor, holds a special spot on that shelf. Selectfluor matters most for a simple reason: it gives working chemists a reliable way to add fluorine atoms to molecules. This reaction—electrophilic fluorination—might sound abstract, but it finds a place in research papers, industry projects, and pharmaceutical design all the time.
Fluorination has gained steam for decades, and not just because it sounds futuristic. Adding fluorine can tweak a drug’s metabolism rate, improve its stability, or bump up its biological activity. Engineers designing new PET imaging agents or disease therapies look for agents that let them introduce fluorine without bringing a lot of safety baggage or tricky handling. Traditional ways of fluorinating things gave a lot of headaches—think harsh gases or unstable compounds. Selectfluor appears less intimidating. It’s a crystalline solid, easier to weigh and use on the bench. The risk feels lower, so more teams feel comfortable reaching for it regularly.
In practice, using Selectfluor means researchers can skip complicated protection and deprotection steps that eat up time. Direct fluorination turns out faster and more straightforward with this reagent. Medicinal chemists see the value firsthand: swapping out a single hydrogen for fluorine sometimes transforms a promising molecule into a blockbuster drug. You see this in the number of fluorinated compounds approved for therapy in the last decade, according to FDA data. More than 20% of modern pharmaceuticals contain fluorine. Drugs like the HIV treatment efavirenz or the cancer therapy sorafenib use fluorination to boost performance. Selectfluor greases the wheels behind these discoveries.
Working in the lab, easy handling makes a difference. Selectfluor doesn’t release noxious fumes or demand expensive ventilation. That changed the game for small labs without huge budgets. The main issues pop up with selectivity. Sometimes the reagent hits more than one spot on a molecule, creating unwanted byproducts. That burns time and hammers project budgets. Researchers look for solutions—asymmetric versions, better catalysts, or greener solvents—each year, drawing from both academic innovation and drug company investment. Recent papers suggest metal-based additives can nudge the reaction toward single-product outcomes, but the hunt for universality continues.
I see Selectfluor as a reminder that innovation isn’t just about raw power or technical leaps. Usability and safety count just as much. University labs, startups, and big pharmaceutical outfits all reach for this reagent because it fits into daily routines without fanfare or elaborate prep. Streamlined chemistry doesn’t just speed up research: it makes progress less dependent on risk and specialized infrastructure. Access levels the playing field. One simple bottle can open up complicated chemistry to folks who otherwise wouldn’t touch it.
Many chemists want safer, more sustainable reagents. Selectfluor shows the direction things can move, but even better options likely exist on the horizon. I talk with students who expect—and press for—less hazardous solvents, higher atom economy, and minimized waste streams. The quest for ideal fluorination tools may not end soon, but the next chapter builds on solid, practical advances like Selectfluor. That’s something any hands-on chemist can get behind.
Storing chemicals never feels routine, at least not after seeing what can go wrong in a poorly ventilated stockroom. Temperature swings, light exposure, and air humidity don’t just look like minor factors on a Safety Data Sheet. Improper storage leads to degraded compounds, ruined research, or, in the worst cases, dangerous incidents. Everybody in a lab or warehouse has stories about bottles splitting their sides or powders that yellowed overnight. Instead of treating “room temperature, dry, and dark” as generic advice, experience shows that small lapses in vigilance can cost real time and money.
Most chemicals fare best between 15-25°C, but it pays off to keep a calibrated thermometer handy. Even compounds classified as “stable” may decompose if subjected to unexpected heat spikes. Peroxides, nitrites, and volatile solvents turn hazardous with just a few degrees above their threshold. In the worst summer days, rooms close to uninsulated windows grow into micro-saunas, pushing sensitive compounds to break down faster or pressure inside bottles to rise. Temperature logs help flag risks before product loss or lab cleanup becomes necessary. Refrigerators and freezers labeled for chemicals—not food—make a difference for sensitive organics, biological samples, or pharmaceuticals.
Light breaks down more chemicals than many realize. Some white powders take on a yellow tinge if they see daylight for even a few minutes. Amber glass and opaque boxes work, but storing them deep inside cabinets with doors shut always feels safer. My first ruined sample came from a bottle left on a bench under fluorescent lights. Humidity brings another layer of challenges. Desiccators and moisture-absorbing packets aren’t just accessories for the most sensitive reagents. Even “stable” salts like sodium chloride form lumps in damp conditions. Fungal growth in corners of shelves often signals a wider storage issue, not just poor housekeeping.
Mixing storage for acids, bases, flammables, and oxidizers creates accidents waiting to happen. A simple shared shelf leads to unintended reactions if a bottle leaks or breaks. Labels and color coding work up to a point, but everybody learns which compounds need their own corners—especially after seeing acid vapors corrode metal shelving or hearing hissing from a spill. Proper distance between groups of chemicals, along with clear signs, keeps daily routines much less stressful.
Every storage method counts on its container surviving the test of time and chemistry. I’ve seen glass crack from pressure or incorrect caps, and plastic can deform if solvents start to eat through their walls. Double-checking seals sounds tedious but spots hazards before they escalate—solid proof that extra attention on routine checks makes accidents rare. Expired or bulging containers must go before they become a source of leaks or contamination.
Logs of storage conditions, regular inventory checks, and labels listing both hazards and dates make every step smoother for new staff and seasoned chemists alike. Posting quick-reference guides near shelves ensures nobody has to guess, and easy access to Safety Data Sheets prevents confusion. Training labs or storage staff to spot early warning signs and follow cleanup routines makes the difference between a minor inconvenience and a costly emergency.
Real-world experience points to one clear lesson: safe, effective chemical storage means more than following broad recommendations. Paying attention to temperature, humidity, light, and segregation saves resources and keeps everybody safe. Regular inspections and simple, clear labeling reinforce safe habits that last. Investing time and equipment into proper compound storage rewards everyone—by protecting both the science and the people doing it.
Products that appear harmless can sometimes surprise you. Take common household cleaners, for example. A bottle of bleach or ammonia can pose real risks if not treated with respect. Stories about accidents involving mixing chemicals pop up more than we care to admit. A friend once landed in the ER after combining bathroom products, not realizing the chemical reaction could send off toxic fumes. Those warnings on the label mean something—ignoring them can have painful and expensive consequences.
Many people still think “special handling” only matters if you work in a lab or a factory. The reality feels different when you unpack a shipment for a new job and find yourself coughing from a dusty cloud leaking out of torn packaging. Eyes sting, skin burns—these are real reactions from common cleaning materials, pool chemicals, or pest control solutions you thought you knew. Training matters, but so does personal awareness. Reading beyond the front label, checking for pictograms, and understanding storage instructions can save you regret—and a call to poison control.
Some products need gloves, goggles, or even dedicated rooms. This isn’t overkill. Chemicals like lye, acids, or heavy solvents in everything from drain cleaner to acrylic paint stripper have a record of causing injuries when handled carelessly. Burns, blindness, and lung damage are not just rare outcomes—they happen every year to thousands of people. The U.S. Consumer Product Safety Commission tracks hundreds of thousands of emergency visits tied to household chemical exposure. The numbers only rise as new formula blends and “super-strength” versions become more popular.
You can catch the signs early. Strong odors, warning symbols, or instructions to “use in a well-ventilated area” all point to something more risky than ordinary soap and water. If you see the skull and crossbones, an exclamation mark, or a burning hand pictogram, these are not for show. They should trigger a plan—like reaching for gloves, finding a mask, opening windows, or avoiding open flames and sparks.
It doesn’t take a technical background to take the right precaution. I’ve seen decent people wind up with blistered skin because opening a container was seen as a quick task. Rushing or getting comfortable with routine often causes the worst accidents. A few seconds spent reading instructions or spending a couple of bucks on some gloves has paid off for me countless times, whether fixing a leaky pipe with solvent cement or scrubbing mildew with strong bleach.
Manufacturers could put clearer, larger warnings or even simple graphics on high-risk products. Stores could place hazardous materials in sections where trained staff can answer basic questions before purchase. Schools and job sites could teach not just the technical details of a product, but the stories behind accidents—these stick with people long past a dry safety video.
At the end of the day, nobody plans to get hurt doing chores or home repairs. But that doesn’t change the fact that accidents happen fast. Taking a few smart steps can make the difference—no degree required, just a willingness to read the signs and respect the risks in the products we use every day.
Learning chemistry in college showed me one thing: every detail counts. A molecular formula tells us exactly what elements make up a compound and in what proportion. Without it, there's no way to know if hydrochloric acid is HCl or if someone is handing you water instead. The numbers matter. In a lab, trusting a bottle’s label isn't enough. Checking the molecular formula avoids mistakes that ruin experiments or produce unsafe reactions.
Green chemistry focuses on safety and environmental impact. Even a small miscalculation in molecular weight skews results. The wrong formula can lead to contamination or unexpected fumes. I remember once in a university lab, a mislabeled container caused a classmate to add potassium permanganate instead of magnesium sulfate. The reaction wasn’t just wrong; it became dangerous. Getting the formula and weight right prevents these problems.
Each time a new drug enters the pharmaceutical market, regulators look for the molecular formula and weight. This isn’t just formality. The molecular weight determines how drugs behave in the body. Too large, and a molecule struggles to pass through biological membranes. The formula ensures consistent results across manufacturing lots. The FDA checks these numbers before giving drugs the green light.
Beyond medicine, chemical processes in everything from cleaning supplies to fertilizers rely on precise molecular formulas. Even small errors raise costs and lose confidence among manufacturers and consumers. Food additives often come under scrutiny because tiny differences in chemical makeup completely change health outcomes. Nobody wants to see allergies triggered because of a labeling error.
During a summer internship, I saw firsthand that getting the numbers wrong doesn’t just mean lost product—it means wasted time. Chemists need the correct formula and molecular weight to calculate the concentrations required for reactions or to measure precise dosing in trials. Industry relies on repeatable processes, and one mistake can send a batch straight to waste.
The world depends on these calculations. Agriculture production scales—fertilizer recipes, pesticide application rates—all these rely on accurate chemical identities. Any accidental substitution or error in the molecular formula can contaminate crops or the environment. It’s more than a technical detail. It turns into a public safety concern in a heartbeat.
Schools could invest early in teaching students to double-check formulas and molecular weights. More time could go to hands-on practice and less to memorizing tables. In the industry, digital verification tools and rigorous cross-checking can help avoid slip-ups. Labeling software updated with regulatory databases shortens the gap between data entry and safe operation. Regular audits and training sessions keep everyone sharp.
Asking the right questions about the molecular formula and weight before starting any task builds safe habits. Taking shortcuts or trusting unverified information leads to costly, sometimes dangerous, outcomes. Experience has shown that attention to chemical details pays off across medicine, food, research, and consumer products.
People often ask what solvents a product will dissolve in. Underneath that question, there’s something more important than chemistry trivia. Solubility decides whether a product can do its job, how safe it is to handle, and how it fits into daily routines at work or around the house. Take common painkillers, cleaners, or hobby materials—understanding the solvents behind these products shapes real decisions, from lab technicians to everyday folks fixing a squeaky door hinge.
I remember working with acrylic paints and learning the hard way that water only goes so far. No amount of scrubbing with water would lift dry paint from a shirt or palette. Someone finally pointed out isopropyl alcohol is the trick. If I had known what my material was soluble in, I might have saved a few shirts and several precious weekends. People deal with similar messes every day, not only in art but with adhesives, inks, or even garden products.
Not every product makes clear what it can dissolve in. For example, toluene and acetone break down many paints and glues, while water stands powerless. Nail polish remover (acetone), paint thinners (mineral spirits), and simple soap each work because the product being dissolved matches with a similar kind of molecule. It’s about the old “like dissolves like” rule: polar solvents (like water) handle polar substances; nonpolar solvents (like hexane) do the job for oils and waxes.
The big problem appears when folks guess about solubility. Mixing chemicals without knowing if they’ll combine safely risks everything from ruined clothes to fires or toxic fumes. The EPA and Consumer Product Safety Commission have warned for years about home cleaning mishaps—mixing bleach and ammonia gives off dangerous gas, but people only learn this lesson after a scare or a trip to the ER.
Trustworthy information doesn’t just land in your lap. The CDC, NIH, and chemical manufacturers keep comprehensive safety sheets. These lists show clearly which solvents handle each ingredient, from prescription drugs to household cleaner. One 2022 study from the Journal of Chemical Education found only 38% of undergraduates could tell water-based from oil-based solubility—even after a standard introduction to chemistry. That means most users need reliable, easily available guides.
I’ve faced the same confusion buying glue at the hardware store. One shelf offers five types of glue for wood, metal, or plastics, but labels rarely break down which solvents will soften or dissolve the product later. Instructions get buried or left out. The cost isn’t just a few wasted dollars—broken shelves, ruined finishes, and sticky hands all remind us that knowledge really matters.
Product labels ought to put solvent compatibility where you can’t miss it, even if it crowds out some advertising. Manufacturers should offer QR codes or simple website charts clarifying what dissolves their products and what doesn’t. Public libraries and local schools could host hands-on workshops to lay out some chemistry basics, letting people experiment without risk.
Pharmacists, hardware store clerks, and paint shop staff could train on these points, arming customers with quick answers before they make a mistake out of confusion. Tougher online resources, like dedicated solubility databases, deserve more attention and clearer links from trusted search engines.
Understanding what dissolves a product isn't just for lab coats—it changes decisions at work and around the house. With better access to straightforward solubility information, customers avoid costly errors and stay safer every day. Everyone needs fewer chemical mysteries in their life.
| Names | |
| Preferred IUPAC name | 1-(Chloromethyl)-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane bis(tetrafluoroborate) |
| Other names |
Selectfluor F-TEDA-BF4 F-TEDA TEDA-BF4 1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane bis(tetrafluoroborate) F-TEDA.2BF4 |
| Pronunciation | /ˈklɔːr.oʊˌmɛθ.ɪl faɪvˈluː.ə.roʊ waɪˈdiː.əˌzoʊ.ni.əˌbaɪˈsaɪ.kloʊ tuː pɔɪnt tuː pɔɪnt tuː ˈɒk.teɪn bɪsˌtɛ.tɹəˌflʊr.oʊˈbɔːr.eɪt/ |
| Identifiers | |
| CAS Number | 140681-55-6 |
| Beilstein Reference | 89868 |
| ChEBI | CHEBI:140497 |
| ChEMBL | CHEMBL3702088 |
| ChemSpider | 113802 |
| DrugBank | DB11274 |
| ECHA InfoCard | 03bfcbd3-7de3-4a90-949d-85c7f166006f |
| EC Number | 63827-81-0 |
| Gmelin Reference | 60462 |
| KEGG | C16685 |
| MeSH | Dichlorofluoresceins |
| PubChem CID | 10442247 |
| RTECS number | GQ0870000 |
| UNII | R8MT53M6XU |
| UN number | UN3277 |
| CompTox Dashboard (EPA) | DJXPZGHSHMZBKE-UHFFFAOYSA-N |
| Properties | |
| Chemical formula | C7H14B2ClF9N2 |
| Molar mass | 323.93 g/mol |
| Appearance | White to off-white powder |
| Odor | Odorless |
| Density | 1.69 g/cm³ |
| Solubility in water | soluble |
| log P | -4.3 |
| Acidity (pKa) | -0.6 |
| Basicity (pKb) | pKb = 6.98 |
| Magnetic susceptibility (χ) | NA |
| Refractive index (nD) | 1.460 |
| Viscosity | 29 cP (20 °C) |
| Dipole moment | 4.77 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 655.6 J·mol⁻¹·K⁻¹ |
| Pharmacology | |
| ATC code | N01AX17 |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes severe skin burns and eye damage. Causes serious eye damage. |
| GHS labelling | GHS02, GHS05, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H302+H312+H332, H314 |
| Precautionary statements | P264, P280, P302+P352, P305+P351+P338, P332+P313, P337+P313, P362+P364 |
| Lethal dose or concentration | LD₅₀ (oral, rat): 114 mg/kg |
| LD50 (median dose) | LD50 (oral, rat) > 2000 mg/kg |
| NIOSH | WF6300000 |
| PEL (Permissible) | PEL (Permissible exposure limit) for 1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane Bis(tetrafluoroborate) is not established. |
| REL (Recommended) | REL (Recommended): **No REL established** |
| Related compounds | |
| Related compounds |
1-Bromomethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane bis(tetrafluoroborate) 1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane chloride 1-Chloromethyl-4-fluoro-1,4-diazoniabicyclo[2.2.2]octane fluoride |
