The journey of trifluoro(piperidine)boron traces back to the rise of organoboron chemistry in the latter half of the 20th century. As industries demanded more robust and unique catalysts and materials, chemists began marrying fluorinated groups with heterocyclic amines like piperidine, then introducing boron to see what would happen. My own early days in the lab came just as the fluorine rush started driving innovation. From the eighties into the nineties, synthesis methods grew smarter—rapid solvent techniques replaced batch heating, boron NMR characterization brought sharper verification, and the knowledge from Barluenga and Suzuki cross-coupling reactions became foundational. By the early 2000s, chemists specializing in fluoroorganics saw molecules like trifluoro(piperidine)boron as potential building blocks with far-reaching applications, from fine chemicals to pharmaceuticals. This period cemented the compound's role in the toolkit of organofluorine research.
Trifluoro(piperidine)boron, sometimes labeled as piperidine boron trifluoride complex or TF-PipB, brings together the strong electron-withdrawing trifluoromethyl group and the ring-stabilized nitrogen of piperidine, bonded with boron. It comes as a colorless to pale yellow crystalline powder or viscous liquid, depending on purity and storage conditions. Chemists know it as more than just another boron donor; it's a useful agent in synthesis, holding court in the realm of selective catalysis and as an intermediate in advanced materials manufacturing. Because of the interplay between boron, nitrogen, and fluorine, the compound shows unique chemical stability under ambient conditions but reacts quickly in designated environments, making it perfect for modern research needs.
This compound weighs in with a molecular formula of C5H10BF3N, and a molar mass of about 168 g/mol. It resists decomposition up to approximately 100°C and shows a moderate vapor pressure at room temperature, meaning storage in tightly sealed, inert containers keeps it in check. The compound dissolves readily in most polar organic solvents—acetonitrile, dichloromethane, and THF—though it prefers staying away from water, as contact typically triggers hydrolysis and diminishes purity. The NMR signature reads distinctly in the boron, fluorine, and nitrogen regions, providing chemists with fast confirmation of identity and purity with relatively little signal interference from common contamination.
Manufacturers set technical specifications based on intended application, with purity standards often above 98%. Labels include not just the CAS number and batch ID, but also recommended storage conditions—below 25°C, away from direct sunlight, and under inert atmosphere like argon or nitrogen. Moisture control proves crucial. Production lots commonly come with certificates of analysis, disclosing not just assay, but also residual solvent content, boron percentage, and spectroscopic data. Transport containers meet UN packaging standards, often using amber glass or Teflon-lined bottles with tamper-evident seals to protect contents from hydrolytic degradation during transit.
Synthesis involves a controlled addition reaction between boron trifluoride etherate and piperidine in dry conditions. The process demands vigilance—glassware must be clean and dry, and the reaction runs best at low temperatures to maximize selectivity and limit polymerization byproducts. In practice, labs use dropwise addition of BF3·OEt2 to a chilled solution of piperidine under nitrogen. The mix is stirred until the reaction completes, which takes about 2 to 4 hours, followed by solvent removal and crystallization steps. Any remaining impurities are handled by repeated washing and filtration, and experienced chemists know to monitor progress by frequent NMR checks to avoid unseen decompositions that creep in with subtle color changes.
Trifluoro(piperidine)boron shines as a ligand or substrate in borylation reactions, especially popular in creating specialty aryl boronates for Suzuki-Miyaura couplings. It balances reactivity: stable enough to store, but eager to react with halides and certain transition metal complexes. Modifications include protecting or replacing the piperidine group for steric or electronic tuning, or swapping fluorine atoms to tweak hydrophobicity and reactivity for pharmaceutical or agrochemical uses. Whether applied in cross-coupling reactions with aryl halides or serving as a precursor to advanced organoboron polymers, this compound’s adaptability opens more synthetic doors than most in its class.
Trifluoro(piperidine)boron pops up in catalogs under names like piperidine boron trifluoride adduct and sometimes simply as TF-PipB. Researchers searching supplier sites or chemical abstracts should check alternate spellings and abbreviations—if a synthesis pathway specifies “Pip-BF3” or “Boron Trifluoropiperidide,” the target molecule remains the same. On MSDS sheets, these synonyms clarify product identification, preventing confusion with similarly named boron trifluorides or unrelated piperidine additives.
Handling this compound means respecting its sensitivity to moisture and potential for toxicity. Gloves and goggles come standard, and well-ventilated fume hoods keep inhalation risk low. Any accidental contact with moisture sparks hydrolysis, releasing HF and other hazardous byproducts—prompt clean-up with calcium gluconate gel and neutralizing agents protects lab workers. Long-term storage calls for inert gas blanketing, and waste solvents require capture and neutralization, not down-the-drain disposal. In my experience, training protocols stress not only chemical handling, but also proper glove removal and emergency eyewash access, as fluorinated boron compounds penetrate skin more rapidly than their hydrocarbon cousins. Safety documentation backs up all claims and legal requirements, meeting GHS and local regulations.
Industrial and academic labs alike use trifluoro(piperidine)boron for its versatility in organic synthesis. Its popularity extends into fine chemical manufacturing, microelectronics, and—most notably—the pharmaceutical sector. It serves as a building block for synthesizing boronic acids and esters, which then support drug scaffolding, chemical sensors, or advanced polymers. One standout application lies in coupling reactions to produce materials for OLED displays and custom resins, where the trifluoromethyl group adds both chemical resistance and unique optical properties. Its application in agrochemical development also rises each year, especially where selective fluorination and boron incorporation help tune environmental stability and biological activity in new crop protection agents.
Over the past decade, research on trifluoro(piperidine)boron has intensified, crossing the borders between synthetic organic, medicinal, and materials chemistry. Teams focus on new synthesis strategies for even greater selectivity, exploring microwave-assisted reactions and greener solvents. I recall several collaborative projects involving computer modeling to predict its behavior in catalytic systems; researchers then validated these predictions with real-world batch runs. Another R&D trend involves integrating this compound into more sustainable development cycles—low-waste recovery systems, solvent recycling, and exploring bio-based feedstocks. As new coupling partners and fluorinated backbones appear in pipeline drug compounds, demand for functional boron reagents like this one continues to rise, fueling not just papers but patents and commercial interest.
While trifluoro(piperidine)boron lands on the less acutely toxic end of the boron chemical spectrum, studies show it irritates eyes, skin, and mucous membranes. Chronic exposure or mishandling can leave more long-term effects, especially from residual hydrolyzed byproducts. Toxicity tests in rodents reveal moderate LD50 values, and metabolic studies indicate partial excretion with some organ retention—especially in the liver. In my own workspace, we run regular biological monitoring and enforce rigorous personal hygiene to cut exposure risks. Few studies address environmental fate, but there’s growing interest in tracking its persistence and breakdown products in soil and water, since boron and fluorine both present long-term ecological hazards in high concentrations.
Looking ahead, trifluoro(piperidine)boron promises to play an even larger role as a linchpin in green chemistry, next-generation electronics, and precision drug synthesis. Demand for highly selective, stable, and modifiable boron compounds continues to push innovation, from automated flow chemistry setups that use less solvent, to digital monitoring systems that fine-tune reaction conditions in real time. Funding bodies and industry analysts see steady market growth as the electronics and pharma sectors invest in new products with boron-fluorine chemistry. If synthetic challenges—cost of fluorinated building blocks, waste management, and process safety—see ongoing R&D attention, this compound looks set to anchor a new wave of materials science and molecular design. It stands as a clear example of how old-fashioned hands-on chemistry, paired with modern analytical and environmental sensibilities, keeps a seemingly niche molecule relevant and valuable for the future.
Every so often, someone outside the lab comes across a chemical name like Trifluoro(Piperidine)Boron and wonders whether this is just another lab curiosity or a tool with a purpose. The funny thing about rare-sounding molecules is, sometimes they play a bigger role than their names suggest. Inside the scientific community, this compound finds its stride in modern organic chemistry and materials development, not just as an experiment but as part of the backbone that supports next-generation medicines and electronics.
Everyone wants medicines that work faster, last longer, come with fewer side effects. Drug makers use all sorts of complex building blocks to get there. Trifluoro(Piperidine)Boron sits among those tools in the medicinal chemist’s toolbox. The benefit comes from its structure. The trifluoroborate group helps molecules survive tough reactions and opens the door to creative ways of building larger, more helpful chemicals.
Take cancer treatment. Chemists work day and night to shape molecules that tell cancer cells to stop growing. Some of these potential drugs rely on scaffolds created with the help of boron-based partners. The boron part lets scientists "stitch" molecules together with precision—joining fragile or tricky pieces that would crack under typical conditions. You see this in a field called ‘cross-coupling chemistry,’ a corner of science that’s launched everything from new fever medicines to powerful antivirals.
Chemistry doesn’t stop at medicines. People also use Trifluoro(Piperidine)Boron in the hunt for better electronics and sensors. Modern phones, batteries, and flexible screens wouldn’t exist without unusual materials at their core. Polymers—large molecules long enough to turn pliable or conductive—gain new features with just the right tweak. Adding groups like trifluoroborates helps polymers carry electrical charges, resist heat, or even glow under LEDs.
Researchers search for molecules that can swap out older, heavier, or more expensive components in consumer tech. They need building blocks that help engineer these features directly into plastics or coatings, avoiding unnecessary waste. The piperidine ring in Trifluoro(Piperidine)Boron lends a good amount of stability and behaves predictably with a variety of other lab ingredients.
There’s always a question of safety with specialty chemicals, and responsible labs take this seriously. Boron brings the advantage of less environmental hazard compared to heavy metals like palladium or mercury. Trifluoro(Piperidine)Boron lets researchers run certain key reactions under gentler conditions. That means less energy use and fewer harmful leftovers.
This doesn’t mean every challenge disappears. The supply chain for making trifluorinated reagents isn’t immune to global shortages, and disposal of unwanted byproducts must follow clear guidelines. Innovation turns on creative and safe use as much as on lab victories.
Scientists focus on making the production of this compound more cost-effective by improving manufacturing steps. Companies keep searching for ways to recycle key starting materials. Training new scientists to use modern techniques safely supports wider access without sacrificing quality or oversight.
Building stronger partnerships between academic labs and manufacturing firms speeds up discovery. Open data on chemical safety and environmental impact helps make careful decisions about large-scale applications. Developing safer analogs for key reactions in both medicine and material science gives teams resilience in a changing world.
Trifluoro(piperidine)boron goes by the molecular formula C5H10BF3N and carries a molecular weight of approximately 169.95 grams per mole. This information looks small on paper but means everything in a chemistry-driven setting. In fields like pharmaceuticals, crop protection, or advanced materials research, accuracy in formulas and molecular weights makes the difference between success and a costly setback.
Exact formulas drive dosing, safety checks, and compliance. I spent a few years in a synthetic lab, and frequent questions circled back to “did you check the calculated mass?” or “are you sure about your compound’s identity?” An error in the formula ruins a day’s work or worse, puts a project timeline in jeopardy. Clarity about C5H10BF3N and its weight isn’t just bookkeeping; it keeps chemists from mixing up reagents, helps procurement teams buy the right raw substance, and ensures everyone reports the right data in published research.
Think about the day-to-day reality of a lab using a compound like trifluoro(piperidine)boron. Suppose the label lists the correct molecular weight. The staff weighs out precise quantities for reactions, calculates yields, and crosschecks purity using NMR or mass spectrometry. Even a small typo in the molecular formula could throw off the data, delaying progress and even risking an experiment's safety profile.
Keen-eyed regulators check everything. Cross-referencing a compound’s structure and molecular weight against registration documents insures against mix-ups. Product labels, safety data sheets, and environmental registrations all trace back to the fundamental knowledge: C5H10BF3N and 169.95 g/mol. Accurate records help investigators retrace their steps if anything goes off-track, from a minor lab spill to a full regulatory inspection.
This attention to detail filters down to things like inventory control and shipping paperwork. Laboratories and manufacturers rely on these numbers for shipment declarations, hazardous material coding, and customs documentation. Even packaging relies on the correct molecular data to decide how tightly to seal, how to store, and how to dispose of excess product.
A lot of new chemical research relies on turning theoretical molecules into safe, workable substances. For trifluoro(piperidine)boron, ongoing studies look at how boron can add value to pharmaceutical design, offering unique reactivity and bioactivity. None of that progress happens unless the people handling these molecules keep close tabs on precise weights and correct formulas. I remember whole team meetings spent parsing the formulae and weights of new compounds before ever touching a pipette.
To close gaps and avoid confusion, it helps to standardize messaging. Keeping the molecular formula and mass visible on reports, containers, and databases avoids missteps. Scientists and technical staff should ask new suppliers to certify data before introducing a new lot of trifluoro(piperidine)boron, and more institutions could use independent quality checks to verify these essentials for every delivery.
Sharing verified molecular formulas and weights in public-facing databases makes life easier for chemists, suppliers, and regulatory officials. It’s not just bureaucracy. In the end, trustworthy data supports research breakthroughs, keeps work environments safer, and guards against surprises—something anyone investing time, money, or health in a complex chemical like trifluoro(piperidine)boron can appreciate.
If someone asks people in a regular lab what product keeps them up at night, not everyone jumps straight to Trifluoro(Piperidine)Boron. Still, it’s the sort of specialty chemical that rewards anyone who thinks about storage from day one. Poor planning can spell ruined product, lost money, and serious safety headaches. Speaking from a background in handling chemicals that refuse to play nice, I’ve learned shortcuts get expensive fast.
This compound combines the firepower of boron chemistry with elements that give it both value and volatility. Plenty of researchers love the reactivity, but that same property makes it a liability on the shelf. Trifluoro(Piperidine)Boron attracts moisture like a sponge; it doesn’t take long before you notice a color change or a weird residue. That's nature’s way of announcing that your reagent’s lost its edge. Beyond performance loss, the bonus risk of exothermic reactions or decomposition makes half-measures risky business.
I’ve always found storing this chemical inside a tightly-sealed, chemically resistant vessel works much better than relying on glass alike to low-value compounds. Polyethylene or PTFE-lined containers block moisture sneaking in. Never cut corners on the liner or gasket—a small leak can write off an entire supply batch. Keeping product integrity means zero gaps for humidity.
Forget the flamboyant “ambient” storage myth. Room temperature does not cut it for Trifluoro(Piperidine)Boron. My go-to method puts this compound in a dedicated fridge set well below standard lab temps. Not the household fridge, either—dedicated flammables storage with temperature monitoring and a clear log of every access. Too many labs ignore daily fluctuation from propping the door open or careless handling. Those extra degrees can make all the difference.
This chemical barely tolerates oxygen. Opening the jar in open lab air for a last-minute bench session goes against good sense. Working in a glove box flushed with dry nitrogen, or at minimum opening under a protective inert gas flow, preserves sample purity and makes an awkward air-sensitive spill less likely. I’ve seen entire years of work derailed by a ten-second lapse in discipline at this step. A forty-dollar cylinder of nitrogen saves four thousand dollars of chemical stock.
Staff turnover, rotating students, lost notebooks—these are the enemies of good storage practice. I make it a point to label every container with full details: purchase date, most recent opening, current storage conditions, and a reminder of handling risks. Digital inventory systems beat out pen-and-paper logs for accountability. It helped me spot trouble before things got costly. Regular training, rehearsed emergency plans, and clear labeling give everyone on the team confidence to act decisively instead of hesitating at the worst moment.
Smart storage for Trifluoro(Piperidine)Boron isn’t just about rules on a safety poster. This discipline stretches budgets, safeguards research progress, and protects people from unplanned exposure or loss. Every lab I’ve seen with a culture of proactive storage ends up ahead in both results and safety records. Chemical handling never gives second chances, but focused attention up front pays lifelong dividends.
People see a complex name like Trifluoro(Piperidine)Boron and worries start piling up. Chemists work with thousands of substances, but most folks have never heard of this one, and the unfamiliar tends to set off alarm bells. I remember learning in a university lab that anything with “fluoro” or “boron” deserves a closer look. Both elements show up in toxic compounds—think of industrial chemicals that damage lungs or cause confusion if handled carelessly. That instinct to treat such molecules with respect hasn’t failed me yet.
Hazard data for this specific compound won’t fill a bookshelf, but we can draw useful clues from its building blocks. Piperidine is a basic chemical found in some medicines, but also known for its strong odor and skin-stinging touch. Trifluoro groups, packed with fluorine, show up in materials that can harm tissues and resist breaking down in the environment. Boron, in controlled doses, helps plants and crops grow, but exposure to larger amounts in certain chemical forms can cause serious health issues.
Research papers on related boron-fluorine compounds mention potential for skin burns, eye damage, and lung irritation. If a lab releases even a small vapor cloud of this kind, anyone nearby might cough for hours. Personally, I’ve seen what happens in a research setting when a new fluorinated compound leaks—a race for the emergency shower isn’t something a chemist forgets. So far, I haven’t seen safety data sheets that label Trifluoro(Piperidine)Boron as “safe.” Instead, any use gets marked with warnings about gloves, goggles, and good ventilation.
Recent years have brought more focus on persistent chemicals—think PFAS, the “forever chemicals” that show up in water and wildlife. Fluorinated boron compounds can’t be assumed safe for streams or soil just because not many studies have tested them yet. It’s a real risk when companies make or ship these materials in bulk. Spills or leaks could mean a local water supply faces years of cleanup. Stories from the field suggest even small errors bring headaches: one colleague spent half a day in a suit, cleaning up after an unnoticed splash dried on a bench.
Lab training should drill in the risks of chemicals with tricky names, not just those with skull-and-crossbones on the bottle. Every new compound deserves a review—correct gloves, fume hood checks, and real discussions about safer alternatives. Regulators do their best to keep watch, but sometimes oversight lags behind new chemical inventions.
Safer handling guidelines work when followed closely. This means clear labeling, up-to-date instructions, and regular hazard drills. Digital safety records cut misunderstandings, especially if everyone on the team has quick access. Producers may explore less hazardous alternatives for industrial processes. If safer chemicals substitute Trifluoro(Piperidine)Boron in research or manufacturing, fewer emergency calls reach poison control hotlines.
Even if most people never touch this compound, they rely on those who do to keep risks contained. Trust builds through honesty and transparency. From the lab bench to wastewater treatment plants, each step to lower hazards adds up. While this chemical’s full story hasn’t been written, handling it with healthy caution and respect keeps both workers and the public safe.
Trifluoro(piperidine)boron sounds complex, but chemists have good reason to keep an eye on it. This compound isn’t a household name, yet it’s creating ripples in the world of synthetic chemistry. Chemists use it as a reagent, especially for adding new pieces to molecules—a process that pushes drug discovery and materials science forward. The sharp minds in labs across the globe recognize its ability to handle selective transformations, and that trust comes from years of practical work, public data, and sharing results in journals.
Drug hunters constantly look for ways to patch together molecules that unlock new treatments. Trifluoro(piperidine)boron helps with that by acting as a kind of “molecular connector.” It often steps in during cross-coupling reactions, an approach honored with the Nobel Prize in Chemistry back in 2010. These reactions matter because they let researchers snap building blocks together in creative ways. I’ve sat through lectures where medicinal chemists light up as they explain how such connectors open doors to molecules that other reagents can’t easily reach.
Cross-coupling using organoboron agents, including the trifluoro variant, provides good yields with a range of functional groups, even those sensitive to metal catalysts. This lets researchers tinker and build new drug candidates or materials for electronics, all while reducing dust-ups with unwanted byproducts. The piperidine piece adds an extra twist—its nitrogen brings flexibility, and the trifluoro groups give resistance to breakdown. That combo sometimes makes the difference between a compound that breaks down fast and one that lasts long enough to become useful.
Pharmaceutical companies don’t just stay in paperwork and test tubes—once a new tool works, they bring it to the plant floor. Trifluoro(piperidine)boron helps pharma manufacturing pull off scale-ups that might stall out with less reliable agents. It finds roles in processes where efficiency and fewer side products mean serious savings. Those who work in chemical process teams look for these little boosts, because shaving off a step, or swapping out a toxic ingredient for a safer one, carries weight—not just dollars, but worker health and less impact on the environment.
Besides pharmaceuticals, some specialty material makers bring in this compound for advanced polymers. Imagine resins meant for electronics or coatings engineered to survive harsh weather; such products depend on the backbone chemistry pioneered in the lab. A tweak using this boron compound might give the finished product improved heat resistance or chemical stability. That matters to engineers, technicians, and end users who count on stuff working longer or safer.
Chemists, both research and industrial, keep a watchful eye on reagents that might turn nasty if mishandled. Trifluoro(piperidine)boron, despite its perks, calls for respect—proper storage, venting, and handling protocols stay high on the priority list. Regulatory agencies demand proof that exposures stay low and disposal follows rules, with guidance coming from studies and workplace experience. Between chemical safety training and responsible sourcing, teams can get the benefits without tradeoffs that threaten people or the planet.
As new findings build up, researchers keep publishing, reviewing, and benchmarking results. Open data on compound behavior, toxicity, and manufacturing improvements helps everyone in the supply chain—scientists, workers, and policy setters—work smarter and safer. The future here depends on real collaboration and honest sharing of both the wins and setbacks.
| Names | |
| Preferred IUPAC name | Trifluoro(piperidin-1-ium)borate |
| Other names |
Piperidinetriyltrifluoroborate Trifluoro(piperidine)boron Piperidine, trifluoroboryl- Piperidine trifluoroborane |
| Pronunciation | /traɪˌflʊə.roʊ.paɪˈpɛr.ɪˌdiːn.bɔːˈrɒn/ |
| Identifiers | |
| CAS Number | 1415326-39-0 |
| 3D model (JSmol) | `3D model (JSmol)` string for **Trifluoro(piperidine)boron**: ``` B1(N2C(C3CCNCC3)C2)(F)(F)F ``` *(This is the **SMILES** string representing the structure, which JSmol can use for 3D visualization.)* |
| Beilstein Reference | 1907486 |
| ChEBI | CHEBI:141360 |
| ChEMBL | CHEMBL4445371 |
| ChemSpider | 11671737 |
| DrugBank | DB14624 |
| ECHA InfoCard | 222-020-5 |
| EC Number | Not allocated |
| Gmelin Reference | 82854 |
| KEGG | C18670 |
| MeSH | D000072964 |
| PubChem CID | 122486804 |
| RTECS number | XZ4825000 |
| UNII | 75Q8Y1056D |
| UN number | UN3334 |
| CompTox Dashboard (EPA) | DTXSID50932460 |
| Properties | |
| Chemical formula | C5H10BF3N |
| Molar mass | 156.0 g/mol |
| Appearance | White solid |
| Odor | Odorless |
| Density | 1.37 g/mL |
| Solubility in water | Solubility in water: reacts violently |
| log P | 1.65 |
| Acidity (pKa) | 2.4 |
| Basicity (pKb) | 3.05 |
| Magnetic susceptibility (χ) | -53.14 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.387 |
| Dipole moment | 3.59 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 273.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1072.83 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1851.7 kJ/mol |
| Pharmacology | |
| ATC code | N05AX10 |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H335 |
| Precautionary statements | P264, P280, P305+P351+P338, P337+P313 |
| NFPA 704 (fire diamond) | 1-3-0 |
| Flash point | Flash point: 71°C |
| NIOSH | *DT8850000* |
| PEL (Permissible) | No OSHA PEL established. |
| REL (Recommended) | 0.05 ppm |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Trifluoro(morpholine)boron Trifluoro(azepane)boron Trifluoro(pyrrolidine)boron Trifluoro(dimethylamine)boron Trifluoro(diethylamine)boron |
