© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
The story of sodium tetrakis(4-fluorophenyl)borate dihydrate started with the hunt for stable, weakly coordinating anions in the field of organometallic chemistry. Chemists dug deep into phenylborate families through the latter part of the 20th century, searching for a compound that could serve as a solid, reliable partner to transition metals without hogging the spotlight in catalytic reactions. The addition of fluorine atoms at the para position of the phenyl rings changed the game. This small structural tweak, paired with sodium as the cation, handed the scientific community an anion capable of getting out of the way enough to let metal centers shine during tough chemical transformations. Researchers soon incorporated the dihydrate form to guarantee practical storage and handling, as water of crystallization helped stabilize the salt in the lab.
Sodium tetrakis(4-fluorophenyl)borate dihydrate lands on the lab bench as a fine, almost white or off-white powder. The compound features a central boron atom surrounded by four 4-fluorophenyl groups, with sodium ions providing charge balance and two molecules of water sitting tight in the lattice. Chemists pick up this salt for its strong utility as a counterion in a range of studies, especially in organometallic syntheses, electrochemistry, and advanced catalysis. This is not the sort of compound you’ll find in everyday products or consumer materials, and it rarely makes the headlines outside academic journals. Yet its role behind the scenes, quietly enabling fundamental discoveries, should not be overlooked.
You can tell a lot about this salt from its solid appearance and the way it handles air and moisture. Sodium tetrakis(4-fluorophenyl)borate dihydrate shows good stability at room temperature in typical lab settings, provided you keep the cap screwed on and store it in a dry place. The salt dissolves in polar organic solvents like acetonitrile, and finds partial solubility in water thanks to its sodium tag, though the big organic anion mostly prefers organic environments. The molecular formula comes out to C24H14BF4NaO2·2H2O, tipping the scales at around 490 grams per mole. Its melting point sits up near 300°C where it tends to decompose rather than slipping into the liquid phase, a trait that hints at its robust structure. UV-spectra show clear absorptions from the aromatic phenyl groups, and NMR signals provide unmistakable evidence for the fluorine atoms in place.
Lab supply companies package this salt in tightly sealed, moisture-resistant bottles. Standard labeling lists sodium tetrakis(4-fluorophenyl)borate dihydrate with clear CAS registry numbers for swift identification. Suppliers note purity of at least 97% or higher for research work, offering batch-specific data sheets that spell out storage conditions, recommended handling, and shelf-life expectations—usually several years if dry and cool. Many labs log hazard statements about eye or skin irritation, keeping guidelines for eye protection, gloves, and working in fume hoods within arm’s reach. In line with international shipping rules, the packaging keeps powder contained even during rough transport.
Making sodium tetrakis(4-fluorophenyl)borate dihydrate calls for stepwise assembly; this is not a one-pot miracle. Chemists start with boron trihalides such as BCl3, treating them with four equivalents of 4-fluorophenyl Grignard reagent under inert gas. After careful work-up to remove magnesium salts, the crude borate anion emerges. Introducing sodium ions lets the solid salt crash out in organic solvents. Adding controlled amounts of water to the dried product yields the stable dihydrate. Each stage of the process brings its own hazards, owing to the use of organometallic reagents and moisture sensitivity, so process controls and good housekeeping in the lab pay dividends.
Chemists value this salt for its “spectator ion” qualities. It won’t leap into most organic transformations, instead letting the spotlight fall on reactive cations like transition metals or main group elements. Transmetallation reactions with silver salts help exchange sodium for less interfering cations, a move beloved in catalysis. The fluorinated phenyl rings refuse to take part in common side-reactions, so the overall structure stands up to moderate acids, bases, and even mild oxidants. For researchers who crave alternatives, tweaks like swapping in different halogen substitutions or using potassium instead of sodium adjust physical properties without overhauling fundamental chemistry. Such modifications, while rare, show how the field tries to tune solubility or reactivity for the next generation of applications.
You might catch this compound under a few names depending on the catalog: sodium tetrakis(4-fluorophenyl)borate dihydrate; sodium tetrakis(4-fluorophenyl)boron; sodium tetraphenylborate, tetrafluoro analog; and less commonly as sodium (4-fluorophenyl)4-borate dihydrate. Most reputable chemical suppliers keep to IUPAC recommendations, keeping confusion to a minimum. Scientists double-check CAS numbers and structural depictions before ordering, since mix-ups with regular tetraphenylborate can trip up even seasoned researchers.
Chemical safety professionals flag this salt for careful handling, much as with other borate and fluoro-organic salts. Most folks in the field use gloves and safety glasses during weighing and solution prep, respecting the potential for mild irritation on skin or mucous membranes. Fume hoods rule the day for any operation with dusts or organometallic byproducts. While not acutely toxic by inhalation or skin contact, the compound still sits on the shelf classified as “handle with care.” Emergency spill kits stay close at hand; boron-containing dust gets swept up wet and disposed with chemical waste, since dust clouds want no place in an indoor lab. The dihydrate also wants no heat or flame thanks to the risk of decomposition at high temperatures. Current standards build from REACH and OSHA guidelines, and institutional Environmental Health & Safety offices confirm best practices without exception.
True value for sodium tetrakis(4-fluorophenyl)borate dihydrate emerges in the world of inorganic and organometallic research, and in the rapidly evolving fields of catalysis and electrochemistry. Electrochemists run to it for its ability to stabilize large cations in solution without complicating redox behavior, fine-tuning delicate measurements in non-aqueous solvents. Organometallic chemists rely on it as a counterion that leaves transition metal catalysts “naked” and ready to work—crafting new reactions for organic synthesis, polymer science, and even cleaner fuel technologies. Beyond these corners of the lab, it rarely pokes its nose into commercial manufacturing or mass-market goods, but research papers and patents show it continuing to pop up in surprising new settings. Its storied utility reflects the broader movement toward uncovering novel reactivity and pushing the boundaries of molecular science.
Experienced graduate students and postdocs choose sodium tetrakis(4-fluorophenyl)borate dihydrate for deep dives into chemistry that needs reliable, predictable results. In spectroscopy, the salt gives sharp, uncompromised signals, paving the way for real insights into electronic structure. Research into next-gen battery electrolytes now probes its potential for enhancing conductivity and improving cycle life, as less interfering anions often translate to higher performance. Collaboration between academia and small tech startups has driven the design of closely related anions, using insights gained from this salt as stepping stones toward safer and greener chemical processes. Hard data from hundreds of publications supports continued funding and interest, and the compound’s story fits neatly into the search for more sustainable and efficient chemistry.
No seasoned chemist takes shortcuts with toxicity, even with compounds that post a low acute hazard rating. Investigations into sodium tetrakis(4-fluorophenyl)borate dihydrate have found low uptake through intact skin and little inhalation risk when handled as designed. Oral LD50 values land well above those for more notorious borates, and the fluorine atoms refuse to detach and build up like some environmental fluorinated hazards. Still, long-term exposure studies remain rare, and the prudent approach means keeping all work in ventilated, clean areas, minimizing contact and seeking medical help for any accidental exposure. Environmental fate studies publish slow but positive news: the salt tends to persist only in controlled, isolated settings, since its organic component likes to bind tightly rather than leach into groundwater or air.
Chemistry never stays still, and new uses for sodium tetrakis(4-fluorophenyl)borate dihydrate keep emerging even after decades of study. Startups probing high-tech solutions to recycling rare earths and precious metals experiment with this salt in their separation schemes. Battery scientists look to minimize “ion pairing” problems using weakly coordinating borates as safer, more stable alternatives to classic inorganic salts. As catalysis moves toward fixing CO2 and unlocking plant-based feedstocks, the demand for robust, non-interfering anions could place this salt front and center. Future research circles around tweaking its structure, reducing environmental footprints, and widening the manufacturing pipeline to make these vital supporting players more accessible worldwide. Investment in green chemistry seeks ways to optimize the synthesis as well, using less hazardous reagents and better waste management strategies. Outreach and collaboration between chemical safety experts and bench scientists help teach the next generation how to work safely and smartly, keeping this pillar of chemical research squarely in the mix for years to come.
People rarely hear about tetrakis(4-fluorophenyl)borate sodium dihydrate outside a lab, but this compound quietly shapes the work of many chemists. Looking beyond the scientific name, many would be surprised to find out how this molecule plays a unique—and sometimes crucial—part in the world of advanced chemistry.
Tetrakis(4-fluorophenyl)borate sodium dihydrate jumped out at me during a graduate class in inorganic chemistry. It showed up right around the same time we tackled problems with ionic liquids and transition metal complexes. The big story, though, doesn’t sit in academic books. This compound often steps in as a non-coordinating anion, one of those oddball helpers that clears the way for sensitive reactions to run cleanly.
Every chemist who's tried to stabilize a reactive cation understands the headaches that come with unwanted interactions. Regular counterions have a habit of "getting involved" in reactions when you least want it. Tetrakis(4-fluorophenyl)borate shines because it sticks to the sidelines. Instead of reacting, it helps hold the positively charged metal or organic fragment in solution, letting researchers make and study compounds that collapse in the presence of most common salts. This property can mean the difference between a breakthrough and a dead end. It’s hard to overstate the importance. Several Nobel-level discoveries leaned on these “innocent” anions to stabilize exotic species that simply didn’t exist before.
This substance shows up in the preparation of weakly coordinating salts, especially in organometallic and catalytic chemistry. Many catalysts in pharmaceuticals, particularly those involving transition metals like palladium or gold, start by pairing these precious metals with stubbornly non-participating counterions. That way, the metal can do its job—activating molecules or stitching together tricky carbon frameworks—without interference from side reactions. As drug molecules grow more complex and expensive, staying away from unwanted byproducts saves time and money.
In electrochemistry, the need for stable electrolytes grows every year. Researchers racing to build better batteries or sensors often turn to salts like tetrakis(4-fluorophenyl)borate sodium dihydrate to set up media that won't short-circuit their work. The stability offered here can lead to clearer results, helping engineers develop devices that serve in everything from small-scale medical sensors to grid-scale energy storage.
Concerns around sourcing specialty chemicals always follow. While few tons leave the lab every year, the environmental footprint of specialty borate salts and associated fluorinated compounds can’t stay ignored. Each synthesis step often involves careful handling and a close look at waste. My own work has led me to weigh up reagent costs and the impact on the waste stream. Researchers and companies must plan disposal and look for greener alternatives wherever possible, especially as regulations tighten around hazardous byproducts.
Some forward-thinking groups keep working to design analogs with less hazardous byproducts or easier synthesis routes. Direct engagement with manufacturers can drive small process tweaks, leading to lower emissions or simpler purification.
Anyone working with new materials, catalysts, or battery technology would do well to learn the ins and outs of these non-classical counterions. The path forward includes better designs, lighter environmental footprints, and a sharper focus on what these supporting actors in chemical reactions can unlock. Collaboration between synthetic chemists and environmental specialists opens the door for more responsible applications, ensuring compounds like tetrakis(4-fluorophenyl)borate sodium dihydrate lift modern chemistry without dragging along avoidable baggage.
There’s nothing like the sting of a chemical splash on your skin to remind you that safety rules aren’t just lab decorations. A lot of people see the warning stickers or read the MSDS sheet and think, “I’m too careful for accidents.” In my experience, accidents don’t ask permission. They sneak up in the middle of a routine task or because you skipped a step, just once. PPE matters, but understanding what you’re holding, mixing, or pouring carries just as much weight.
Chemical labels aren’t just box-checks for regulators. Some chemicals burn through nitrile gloves or eat through old latex. I remember working with strong acids for a demonstration, trusting those thin blue gloves. One drop changed my outlook about double-gloving with the right material. Look for splash goggles, not just safety glasses, and check the seal—goggles lose their tightness as they age. Don’t forget your coat, long pants, and closed-toe shoes every single time.
Breathing fumes might not seem dangerous if you can’t smell or see anything in the air. The truth is, some chemicals can damage your lungs, nerves, or liver long before you cough. Fume hoods draw poisonous vapors away; they’re not optional for volatile substances. Never store acids near bases or flammables near heat. I’ve seen storerooms where bleach sat next to ammonia, an accident just waiting for a bumped shelf.
Panic is the enemy in an emergency. Once, a coworker splashed sodium hydroxide on his arm, but nobody in the room knew where the emergency shower was. That hesitation left him with a scar. Learn the location of eyewash stations and showers. Practice unclipping the clasp, even if it feels silly, so your hands can do it blind. Keep spill kits stocked where they make sense, right near the work—never padlocked down the hall under a “Hazmat” sign.
Book knowledge only does so much. Real safety comes from running drills and talking about near-misses. The best teams I’ve been part of treated safety as a shared responsibility. If you notice a label peeling off, fix it or flag it. If the fire extinguisher sits dusty in a corner, get it checked. It’s not about paranoia—it’s about routines strong enough to catch mistakes before they hurt someone.
It’s easy to slip into autopilot after dozens of routine procedures. The incidents that stick with me the most came from people distracted by deadlines. Safe handling starts with attitude: treat every bottle and drum as if it has bite. Read the SDS, consult the compatibility chart, and lay out all the gear before you open the lid. Safety isn’t a checklist—it’s a habit built one careful action at a time.
TETRAKIS 4 Fluorofenil Borato de Sodio Dihidrato has a name that makes most people reach for an extra cup of coffee before reading the label twice. It’s not a household chemical, but it finds real work in specialized chemical synthesis, sometimes in the labs that help build the foundation for pharmaceuticals and materials science. These are places where you can see the true impact of getting storage and handling right—or wrong.
This compound brings a few quirks to the table: moisture sensitivity, some degree of reactivity, and basic health and safety concerns. Many seasoned chemists learn quickly that the rules of safe storage aren't about being overcautious—they’re about having respect for the chemistry and the risks it brings, both for people and equipment.
One mistake I’ve watched newer lab techs make is thinking a tightly capped bottle on a shelf counts as a solid plan. It doesn’t. Sodium salts like this borate have a sneaky habit of pulling moisture from the air, even if you aren't watching. I’ve dealt with bottles caked with crystals because of exposure, and that’s a red flag both for chemical quality and safety. So desiccators aren’t just for show—they’re critical. Placing the compound in a well-sealed container inside a desiccator with fresh desiccant keeps it dry, stable, and fit for future use. In big research settings, I’ve seen desiccated cabinets with alarms go a long way in keeping everyone out of trouble.
I come from a lab where winter meant battered heaters and summer meant burnt out air conditioners. Temperature swings aren’t good for any chemical we want to keep pure. For TETRAKIS 4 Fluorofenil Borato de Sodio Dihidrato, room temperature is often enough, but “room” means something steady and away from direct sunlight or hot equipment. Shelves at eye level in climate-controlled rooms work best, far from vents or sources of drafts. This isn’t just about preserving shelf life—unstable storage leads to changes in chemical properties, and in my time, that’s opened the door for unnecessary waste and risk.
Mislabeling stands as the simplest mistake with the biggest consequences. A faded label or no record of the opening date makes for accidents waiting to happen. It takes little effort to write in permanent ink—the chemical name, opening date, and hazard information. I’ve watched teams lose weeks over avoidable confusion. A simple barcode system won’t hurt, either, especially with large inventories.
There’s always temptation to fit one more bottle into a storage unit. Crowding borates near acids, water sources, or oxidizers turns minor incidents into big ones fast. Experience taught me to keep isolation the rule. Even in basic stockrooms, chemicals stored with clear separation and in ventilated spaces show fewer corrosion issues and help limit the spread if any spillage occurs.
Fail-safes like regular inspections help. No one likes extra work, but I’ve seen more than one disaster averted just because someone noticed a loose cap or spilled powder on a shelf. Basic PPE like gloves, goggles, and a clean workbench save much more than time: they keep people healthy. Keeping a safety sheet handy, right near the storage area, gives everyone on the team a place to double-check procedures—no need to rely on memory alone.
Small changes like these, learned from digging into daily lab work, can make a real difference, turning chemical storage from a weak link into a source of confidence and reliability for everyone on the team.
Most of us don’t walk into a store thinking about chemical formulas behind what we buy. A phone charger, a cleaning wipe, a deodorant stick—they just line the shelves. But not everything that shows up in your cart finds its way in without potential hidden risks. Growing up, my family tackled stains with bleach and polished wood with sprays that lingered in the air. We usually thought products were harmless if they came from a reputable brand or sat on familiar aisles. Only years later did brands face lawsuits for toxic talc powders and spray cleaners linked to breathing problems.
Labels throw out words like “natural,” “safe for kids,” or “eco-friendly.” In reality, these phrases often hide behind weak regulations or friendly marketing. I once bought an “organic” multipurpose cleaner, only to experience coughing fits every time it hit the tile. Digging into its Safety Data Sheet pointed to sodium hypochlorite—still bleach in another form. That taught me not to judge a bottle by its flower-patterned label.
Across the United States, laws let manufacturers skip listing many fragrance ingredients under the catch-all “fragrance.” A 2018 Environmental Working Group report revealed that one popular air freshener contained phthalates, linked to hormone disruption, though the box made it sound family-friendly. Scientists continue to raise concerns about microplastics, flame retardants, and the way kids’ toys might still carry heavy metals like lead. Even items labeled BPA-free sometimes swap one questionable plasticizer for another.
Full risk disclosure shouldn’t feel like a scavenger hunt. If a cleaner might damage lungs or a plastic container could leach chemicals into food, those facts should be front and center. During a project in college, my lab analyzed water bottles for contaminants. Brands differed wildly in their willingness to tell us what went into their plastics. Some rattled off compliance jargon that didn’t mean much to average families. Others pointed to certifications you practically need a chemistry degree to decode.
Health risks aren’t just personal. Take PFAS—so-called “forever chemicals”—slowly building up in the environment because they don’t break down in water or soil, showing up in rain, fish, and even mothers’ milk. The US Centers for Disease Control and Prevention now tracks levels in people nationwide, flashing signals about potential links to cancer and immune issues. Ignoring these risks lets pollution and chronic health concerns spread quietly.
Swaying industry giants starts with demand from regular people. In the last decade, grassroots campaigns nudged national chains to drop certain toxic flame retardants from furniture, limit bisphenols in receipts, and offer low-VOC paint. Public pressure, lawsuits, and social media have all forced more open ingredient lists.
Policy plays a big part too. Europe's approach, through its REACH regulations, pushes companies to prove ingredients’ safety before wide release. In the US, reforms to the Toxic Substances Control Act forced chemical makers to submit more data for new and existing formulas, but plenty of gaps remain. Looking ahead, supporting tighter standards and transparency fights the idea that it's fine to gamble with health for the sake of market speed.
If knowledge is power, then getting the facts turns today’s cautious shopper into tomorrow’s confident consumer. The more we ask, the more brands tell—and the safer shelves become.
People sometimes underestimate how much a product’s chemical composition can impact health, safety, or even performance. Take sunscreen, for example. The active ingredients absorb or block harmful UV, but not all formulas work the same way. Oxybenzone, a common filter, protects skin, but research from the Environmental Working Group and published studies in JAMA shows traces of it entering the bloodstream after use. Some folks now look for zinc oxide instead, because this mineral-based compound sits on the skin’s surface, forming a physical shield. Knowing which chemicals a consumer rubs onto their skin changes the conversation from just “does this stop sunburn?” to “will this end up inside me, and is that safe?” Real questions deserve straightforward answers.
Ingredients aren’t always easy to decipher. Consider processed foods. Take potato chips: potatoes, oil, and salt seem basic, but turn over a bag and extra components often jump out. Terrestrial flavor boosters like monosodium glutamate (MSG), artificial colors, and anti-caking agents sneak in. The FDA lays out rules for what goes into food, but sometimes companies use umbrella terms like “spices” or “natural flavors.” These categories mask a range of chemicals with trace allergens or compounds some folks choose to avoid. My experience tells me that, for many with allergies or dietary restrictions, hunting for the specific chemical makeup becomes essential—not just a passing curiosity.
Think about cleaning sprays. Many promise a lemony fresh scent, but “fragrance” can mean any mix of hundreds of chemicals. A 2016 study from the University of Melbourne found that even scented cleaning agents sold as “natural” often contain VOCs (volatile organic compounds), which can produce indoor air pollution. Exposure sometimes leads to headaches or rashes. Many consumers with asthma or sensitive skin feel safer after switching to fragrance-free products. If a company named each component, it would make these choices easier, but marketing rarely works that way. People shouldn’t need a chemistry degree to avoid something that makes them sneeze.
Trust happens when companies tell the full story. The rise of regulatory measures like the EU REACH regulations forced companies to publicly share risk data and detailed breakdowns for many ingredients. In the United States, the Personal Care Products Safety Act aims to make formula disclosures clearer. Public databases and digital apps now help ordinary people decode labels, showing links between chemicals and health effects. This trend brings power back into the hands of consumers.
On the research side, independent labs can test samples for their chemical fingerprints. A friend working in environmental science once shared how neighborhood kids tested playground mulch and found high levels of recycled tire chemicals. Their findings helped convince the local council to swap to untreated wood chips. Scientific transparency led to community-led change.
Everyone deserves to know what’s inside the products they eat, use, or touch. Companies that clearly break down chemical structures set themselves apart. Regulators and watchdog groups can keep pressure on, but crowdsourcing and open data build trust, too. By making science less mysterious, we help everyone make wiser, safer choices in daily life.
| Names | |
| Preferred IUPAC name | sodium tetrakis(4-fluorophenyl)borate dihydrate |
| Other names |
Sodium tetrakis(4-fluorophenyl)borate dihydrate Sodium tetrakis(p-fluorophenyl)borate dihydrate NaBArF4·2H2O Sodium tetrakis(4-fluorophenyl)borate hydrate Sodium tetrakis(para-fluorophenyl)borate dihydrate |
| Pronunciation | /ˈtɛ.trə.kɪs ˈkwat.roʊ fluˌɔː.roʊˈfɛ.nɪl boʊˈreɪ.toʊ deɪ ˈsoʊ.di.oʊ daɪˈhaɪdreɪt/ |
| Identifiers | |
| CAS Number | 210265-69-3 |
| 3D model (JSmol) | `/display=JSmolLoad('Na(B(C6F5)4)·2H2O')` |
| Beilstein Reference | Beilstein 4122533 |
| ChEBI | CHEBI:141607 |
| ChEMBL | CHEMBL4207749 |
| ChemSpider | 2944015 |
| DrugBank | DB14754 |
| ECHA InfoCard | 03a2f27c-9633-44af-9a2e-3a1e2a278e25 |
| EC Number | 68259-34-5 |
| Gmelin Reference | 457332 |
| KEGG | C21177 |
| MeSH | D008075 |
| PubChem CID | 139657252 |
| RTECS number | XT2150000 |
| UNII | 006R2K3L4X |
| UN number | UN3467 |
| Properties | |
| Chemical formula | NaB(C6H4F)4·2H2O |
| Molar mass | 406.08 g/mol |
| Appearance | White to off-white powder |
| Odor | Odorless |
| Density | 1.69 g/cm3 |
| Solubility in water | Insoluble |
| log P | -0.3 |
| Acidity (pKa) | 2.9 |
| Basicity (pKb) | 2.8 |
| Magnetic susceptibility (χ) | Diamagnetic |
| Refractive index (nD) | 1.570 |
| Viscosity | 900 - 1100 cP (20°C) |
| Dipole moment | 1.0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 540.5 J·mol⁻¹·K⁻¹ |
| Pharmacology | |
| ATC code | V09AX04 |
| Hazards | |
| Main hazards | Causes skin and serious eye irritation. Harmful if swallowed. |
| GHS labelling | GHS05, GHS07, Danger, Causes serious eye damage, Causes skin irritation, May cause respiratory irritation |
| Pictograms | GHS05,GHS07 |
| Signal word | Danger |
| Hazard statements | H302: Harmful if swallowed. H315: Causes skin irritation. H319: Causes serious eye irritation. H335: May cause respiratory irritation. |
| Precautionary statements | P264: Lavarse las manos cuidadosamente después de la manipulación. P270: No comer, beber ni fumar durante su utilización. P301+P312: EN CASO DE INGESTIÓN: Llamar a un CENTRO DE TOXICOLOGÍA o a un médico si se encuentra mal. P330: Enjuagarse la boca. |
| NFPA 704 (fire diamond) | 2-0-1 |
| Flash point | > 220 °C |
| Lethal dose or concentration | Lethal dose or concentration (LD50/LC50): LD50 (oral, rat): >2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): >2000 mg/kg (oral, rat) |
| NIOSH | WW6475000 |
| PEL (Permissible) | PEL (Permissible): Not established |
| REL (Recommended) | 20 mg/m³ |
| IDLH (Immediate danger) | NIOSH: Not established |
| Related compounds | |
| Related compounds |
Sodium tetraarylborate Sodium tetraphenylborate Potassium tetraphenylborate Tetraphenylborate anion Fluorophenylborates |
