4-Bromofluorobenzene: A Chemist’s Look at an Unsung Workhorse
Historical Development
4-Bromofluorobenzene came on the scene as synthesis methods matured in the early 20th century. Chemists at the time sought ways to tweak the benzene ring with different substituents, aiming to tune reactivity, boiling points, and biological activity. The combination of bromine and fluorine gave a molecule both manageable in the lab and useful for larger goals, particularly as organofluorine chemistry grew up alongside developments in pharmaceuticals and polymers. Early patents from chemical giants like DuPont and Bayer logged several halogenated benzenes, including this one, as researchers chased products for dyes, pesticides, and intermediates. My years in organic synthesis taught me straightaway: once a halogenated benzene gets into the catalog, it tends to stick around because someone will always find another use.
Product Overview
4-Bromofluorobenzene often appears as a lab standard, tucked alongside its cousins in chemical storerooms worldwide. This compound wears a practical hat in organic methodology, acting as both a building block and a testing ground for cross-coupling reactions, especially Suzuki-Miyaura and Buchwald-Hartwig couplings. Chemists prefer it because the bromine acts as an efficient leaving group, while fluorine tunes the electronic character of the molecule, guiding selectivity and reactivity downstream. Any discussion of advanced pharmaceuticals or agrochemical research eventually touches on this compound, since its framework slides so neatly into synthesis flows.
Physical & Chemical Properties
4-Bromofluorobenzene is a clear, colorless to pale-yellow liquid at room temperature. It carries a distinct, pungent odor — one whiff takes me right back to grad school hoods. Density settles just over 1.5 g/mL, and boiling point rides around 151°C, which means most distillations happen under reduced pressure to avoid decomposition and drift. It’s less dense than, say, 1,2-dibromo compounds, which sets it apart in separations. Solubility leans toward organic solvents, barely mixing with water, making it suited to multi-phase reaction conditions common in synthesis labs. Fluorine gently tightens the electron cloud, reinforcing the aromatic ring, while bromine’s mass and size break symmetry, opening doors for selective substitutions.
Technical Specifications & Labeling
Suppliers list purity levels between 97% and 99%, which suits most research and industrial purposes. It generally comes stabilized with a pinch of copper or another trace antioxidant, staving off light-induced decomposition. Specifications include detailed spectroscopic fingerprints: NMR signals around 7.0 to 7.6 ppm in proton NMR tie directly to the aromatic protons, with heavy halogen-coupled splitting. GC and HPLC methods confirm purity, and MS spectra frequently show the distinctive heavy bromine isotopic pattern. Labels and documentation keep hazard statements front and center, as regulations worldwide (REACH, GHS) demand manufacturers disclose risk and provide guidance on safe handling.
Preparation Method
Industrial synthesis usually hinges on electrophilic aromatic substitution, starting with fluorobenzene. Bromination with bromine in the presence of iron or aluminum tribromide edges the reaction toward the para position, taking advantage of that fluorine’s directing effects — a behavior any organic chemist learns by rote. In the lab, smaller batches might use N-bromosuccinimide as a bromine source, dropping in iron filings to keep things moving. Sometimes, aniline analogs are diazotized and then fluorinated and brominated in sequence, depending on starting material price and downstream requirements. Purification generally leans on vacuum distillation or repeated recrystallization from nonpolar solvents if solid binds form on cooling.
Chemical Reactions & Modifications
4-Bromofluorobenzene kicks off Suzuki cross-couplings like clockwork. Every major synthetic lab has run the reaction to drop in boronic acids, building out complex aromatics or polyaryl structures. The bromine leaves under palladium catalysis, while the sturdy C–F survives to steer reactivity further along. Other developers use the molecule as a precursor for nucleophilic aromatic substitution: a basic amine or alkoxide can clip off the fluorine if forced, yielding para-substituted derivatives for more advanced applications. Reduction, metalation, and halogen-metal exchange make frequent appearances too; I saw Grignard reagents prepared from this very molecule lining up for additions on more than one occasion.
Synonyms & Product Names
Chemists recognize it under many guises: para-bromofluorobenzene, 1-bromo-4-fluorobenzene, 4-fluorobromobenzene, and variations in supplier catalogs. Some industry insiders abbreviate it as PFB or use trade names for bulk sales, especially when the compound routes into specialty chemical production. Synonyms help trace back literature records, old lab notebooks, and patent filings, so researchers shouldn’t overlook these minor changes—they often open up search strategies or clarify methods when troubleshooting.
Safety & Operational Standards
Working with 4-bromofluorobenzene means respecting its volatility and irritant qualities. Vapors irritate the eyes and respiratory tract, so the right approach stays rooted in solid lab habits: gloves, goggles, and fume hood always on hand. Safety data sheets call out possible effects on skin and mucous membranes and highlight that long exposures might sensitize or irritate. Some agencies flag the risk of environmental accumulation due to the stability of the aromatic fluorine, so waste solutions collect in designated halogenated solvent bottles for proper incineration rather than casual disposal. Any scale-up includes fire suppression plans; the flash point hovers low enough to raise eyebrows.
Application Area
Most research chemists view 4-bromofluorobenzene as a platform for creating functionalized aromatics. Its value shines brightest in medicinal chemistry—think kinase inhibitors, CNS agents, and imaging agents for PET scans—where rigid frameworks studded with halogens adjust bioavailability and target affinity. Agroscientists rely on it, too, for making crop protection agents. Polymer scientists have used its structure as a monomer or comonomer for high-performance plastics, leveraging the halogen mix to change flame resistance or chemical durability. Electronics manufacturers increasingly look to such functionalized aromatics when tweaking dielectric constants and optical properties in display technologies.
Research & Development
R&D around 4-bromofluorobenzene never slows, partly because the molecule answers tough synthetic challenges. Method developers in catalysis circles love its straightforward substitution pattern: using it in high-throughput screenings uncovers more tolerant cross-coupling protocols and greener reaction conditions. Ongoing studies track its fate in environmental settings, testing for persistence and the possible generation of harmful byproducts. Collaboration between academia and industry keeps focus on developing cheaper, more sustainable manufacturing methods—especially those using renewable feedstocks or low-energy catalysis. At several roundtable workshops I joined, scientists shared firsthand insights into the real, practical pain points of scaling these halogenations and whether photoredox or biocatalysis might edge out traditional metal reagents.
Toxicity Research
Toxicity data for 4-bromofluorobenzene suggest moderate acute hazard, with reported LD50s in rodents ranging between 1,000 and 2,000 mg/kg. It doesn’t rank among the more potent toxins, but chronic exposure remains less studied. Researchers keep a close watch for mutagenicity and bioaccumulation, two red flags in modern hazard assessment. Systematic reviews note mild hepatic and renal stress at high doses. I’ve watched regulatory lines get drawn tighter over decades as more data lean toward caution; today’s labs no longer treat halogenated benzenes as routine throwaways but as compounds deserving scrupulous capture and destruction. Innovative approaches in green chemistry actively seek alternatives or at least provide ways to break down this molecule after its industrial use.
Future Prospects
Looking ahead, 4-bromofluorobenzene stands poised to support both old and new technologies. Drug hunters need small and versatile platforms to build next-generation therapies, and this molecule’s shape and reactivity fit that bill. Demand for safer, more selective pest control also keeps the door open for further modifications and analog development. Advanced materials and nanoelectronics research show no signs of slowing interest, especially with the growing appetite for molecules that engineer electronic properties at the atomic level. Addressing sustainability will mark the big challenge: chemists can push for bio-derived syntheses or closed-loop recycling of aromatic halides to cut environmental load. Each step forward draws on the lessons chemists learned through decades of handling and modifying 4-bromofluorobenzene—reminding all of us that progress depends as much on wisdom and accountability as it does on clever molecules.
The Core Formula: C6H4BrF
Every so often, you run across a compound that seems simple on paper yet holds notable significance in both industry and labs. 4-Bromofluorobenzene, with the formula C6H4BrF, marks one such example. After spending years handling aromatic compounds in the lab, I know the importance of these modest molecules. Every atom in this formula has its own role: six carbon atoms shape the benzene ring, four hydrogens round out the ring's stability, while one bromine and one fluorine bring new properties, from reactivity to changes in boiling point. The arrangement matters as much as the formula. Here, the bromine and fluorine atoms sit opposite each other on the ring, which affects how the molecule behaves in chemical reactions.
Real-World Uses Make the Chemistry Matter
Chemical formulas become more valuable once you see how they show up in tangible ways. Take C6H4BrF—industries rely on it as a building block for pharmaceuticals, agricultural compounds, and specialty materials. Lab technicians use it to introduce both halogen atoms into new molecules, in reactions cleaner than some older routes. I have seen scientists choose this compound for processes demanding both selectivity and efficiency, such as making drug candidates with tricky synthetic requirements.
The heavy bromine atom adds heft to the molecule, making it useful in certain radiolabeling steps, while the fluorine atom contributes both metabolic stability and chemical resilience. Research published in the journal Organic & Biomolecular Chemistry outlines how these characteristics lead to innovative synthetic routes.
Safety Remains a Priority
Knowing the chemical formula only goes so far. Safety practices transform that knowledge into responsible action. 4-Bromofluorobenzene packs reactive halogen atoms, which means it can trigger skin and eye irritation if mishandled. Even though its volatility is lower than some smaller halogenated benzenes, users in both academic and industrial settings wear gloves, goggles, and lab coats. The Globally Harmonized System for labelling chemicals highlights this compound as hazardous, urging proper ventilation even during short tasks.
Mismanagement risks more than personal safety. Accidental releases can contaminate water sources. We've learned from past incidents to never underestimate aromatic halides' environmental reach. Good lab protocol and waste disposal, guided by local safety data sheets, guard against unnecessary exposure. Research labs and manufacturers now take extra precautions in how they ship, store, and handle C6H4BrF, underscoring a broader shift toward chemical stewardship.
Supporting Better Practices with Facts
The best way to support safer chemical work is to spread correct, science-backed data. Studies from agencies like the European Chemicals Agency (ECHA) provide up-to-date recommendations specific to halogenated benzenes, including how long-term exposure might impact health or the environment. Access to this data lets users make informed decisions—choosing the right containment, the right emergency response, the best waste practices. This careful approach doesn’t hold back research; instead, it sets scientists up for cleaner results and fewer risks.
By focusing on the exact formula, understanding usage, and respecting safety data, anyone working with 4-Bromofluorobenzene can balance productivity and responsibility—turning a simple-looking formula into a tool for better science and safer workplaces.
How Chemists Rely on 4-Bromofluorobenzene
Anyone who’s spent time in a laboratory knows the value of having the right building block for each job. 4-Bromofluorobenzene isn’t a chemical you’ll find in a kitchen or pharmacy, but it shows up often on the shelf of synthetic organic chemists. The structure—one part bromine, one part fluorine, both attached to a benzene ring—offers a unique tool for anyone making more complicated molecules.
Years working in a lab taught me the pain of syntheses stalling out due to side reactions or stubborn byproducts. A compound like 4-Bromofluorobenzene gives chemists a way to fine-tune reactivity. The bromine atom makes it suitable for Suzuki and other classic cross-coupling reactions. The fluorine atom can survive a range of conditions, letting a researcher tweak properties—like how a molecule interacts with receptors—without blowing apart the rest of the system.
Drug Development and Pharmaceuticals
Fluorinated chemicals show up all over the pharmaceutical world. Once you start looking, you’ll see them everywhere from anti-cancer drugs to antidepressants. Adding a fluorine atom can improve a drug’s metabolic stability or help it fit better into a biological target. Pharmaceutical scientists reach for 4-Bromofluorobenzene to create intermediates, which then get turned into promising new medicines.
A drug company hoping to develop the next big painkiller, for example, may start with this molecule to introduce fluorine at exactly the right position. One survey in the Journal of Medicinal Chemistry found that almost 20% of new chemical entities hitting the market include at least one fluorine atom. They’re not picking these building blocks at random—they boost a drug’s chances of making it through the gauntlet of animal tests, clinical trials, and regulatory review.
Crop Protection and Specialty Chemicals
Chemists working on pesticides and herbicides see similar challenges. You want a compound that sticks around long enough to do its job, doesn’t break down before reaching its target, and doesn’t cause more harm than good. The fluorine atom helps by increasing the stability and effectiveness of agrochemicals. Companies turn to 4-Bromofluorobenzene for these syntheses, taking advantage of its ability to act as a flexible, reliable intermediate.
In practice, this means safer pest control, better yields, and sometimes lower environmental impact. The role of fluorinated compounds in advanced crop protection grew steadily over the past two decades, especially as regulations forced out older, less selective chemicals.
Advanced Materials and Everyday Technology
Some of the most durable consumer products hang together because of fluorinated compounds. 4-Bromofluorobenzene feeds into the synthesis of materials used in liquid crystals, display technologies, and special plastics. Adding fluorine atoms can give materials resistance to heat or corrosion, which matters for screens, batteries, and cables that need to work in harsh conditions.
The demand for smartphones, flat panels, and wearable tech keeps pushing research into new molecules like this one. These materials didn’t show up by accident: researchers spent years testing thousands of versions to find out which combinations could weather the toughest tests.
Addressing Safety, Sustainability, and Access
The benefits of 4-Bromofluorobenzene come with challenges that shouldn’t get swept under the rug. I’ve handled organobromine and organofluorine compounds. They demand care—exposure risks, specialized disposal, and environmental management add cost and complexity. Reports by the European Chemicals Agency show that regulatory oversight on compounds like these will probably increase.
Continued improvement in process chemistry, greater transparency in the supply chain, and a push for safer handling protocols can help mitigate the risks. Academia and industry have already started sharing greener synthesis methods. As with most specialty chemicals, the best results come from clear communication, strong safety culture, and investment in new research.
What You’re Dealing With
4-Bromofluorobenzene gets used for more than lab experiments. Researchers turn to it in pharmaceuticals and materials preparation, so new tech and medicines can launch. Scanning a bottle on a chemistry bench doesn't reveal the whole story. A colorless liquid rarely hints at the trouble it brings to skin or lungs. Even a whiff or a quick splash exposes you to risks that can last longer than any short lab session. Treating it like water or a friendly solvent puts your safety and the integrity of your work at risk.
Personal Protection Works
Anyone who’s spent long hours in the lab knows gloves matter, but not just any glove stands up to aromatic halides. Nitrile gloves can resist occasional splashes. Thicker ones, changed out regularly, offer better peace of mind. Shortcuts don’t help—you want a fresh pair every time you handle this stuff. A closed lab coat and chemical goggles close the loop. Safety specs, not reading glasses, block what your eyes can’t handle. Long pants and closed shoes finish the outfit because nobody wants to wash chemicals from their socks at the end of the day.
Avoid That Inhalation Risk
People overlook vapors because they don’t see them. These are the dangers that stick with you: headaches, dizziness, and possible lung impairment sneaking up later. I learned fast that fume hoods aren’t decorative. Good airflow draws away tiny particles and vapors before you can take a single breath filled with trouble. This precaution isn’t negotiable. Even pipetting a small volume turns risky in a poorly ventilated spot.
Don’t Bring It Home
Chemicals love to hitchhike out of the lab on sleeves and baggy cuffs. Before grabbing your bag and heading out for lunch, wash up—soap and water, no exceptions. Keeping a dedicated set of work clothes and shoes in the lab area separates your home from the site of your science. I’ve had friends who left work with chemical smells on their jackets, not realizing what they brought into their cars. Changing and washing up gives you control, not fear, when you leave the workspace.
Spill Planning Saves Panic
I once saw panic turn a minor spill into a major problem. Preparation solves most flare-ups. Having a spill kit stocked and ready, with absorbent pads and neutralizers specific to organics, lets you respond instantly. Training isn’t about rule-checking; it means your hands know what to grab before nerves kick in. The difference between a contained spill and an evacuation comes down to practice—everyone involved should get hands-on with their kit before any real event.
Waste and Storage: Details Matter
Disposing of halogenated organics isn’t an afterthought. Dedicated containers with tight lids keep fumes where they belong. Labels must be accurate, not vague, because mixing chemical wastes risks violent reactions. Storage belongs in a cool, well-ventilated spot, away from sources of heat and incompatible reagents. Lax storage turns minor leaks into exposure or even fire risks, especially with volatile compounds.
Knowledge and Respect
Experience shapes the way people approach chemicals like 4-Bromofluorobenzene. Stories from those who ignored protocols show real consequences—hospital visits and permanent scars. Knowledge, not bravado, lays the groundwork for smart decision-making. Take time to read safety data sheets, learn from veteran lab workers, and never treat routine exposure as safe. Respect for the material, colleagues, and your own health pays off long after the workday ends.
Context From the Lab Bench
Anyone who has ever weighed out a white crystalline powder in a chemistry lab understands how a forgotten molecular weight can slow everything down. 4-Bromofluorobenzene might not sound glamorous, but in industry and research, its number matters. This compound packs a bromine atom and a fluorine atom onto a benzene ring, giving it both heft and reactivity.
Students often memorize the periodic table, but people stop and check the numbers when it comes to real quantities. 4-Bromofluorobenzene sports a molecular formula of C6H4BrF. Add up the numbers: Carbon brings 12.01 g/mol each, so six in a ring gives 72.06. Four hydrogens at 1.008 g/mol add another 4.032. Bromine piles on with 79.904 g/mol, and fluorine clocks in at 18.998 g/mol. Their sum is 174.99 g/mol, usually rounded to 175 g/mol.
Why This Number Matters
Nobody likes to talk about saving time by knowing a number, but in synthesis, every minute you aren’t fiddling with calculations keeps your reaction on track. If you overshoot on brominated compounds, you can wreck a synthesis. Too little and you waste precious hours. The molecular weight grounds your entire calculation—milligrams scale up to kilograms in pharmaceuticals, dyes, and agrochemicals. A single error infects the whole process. In my own grad student days, I ran a handful of blank tests because I’d swapped a reagent and flubbed the math. Lost a day to a typo.
Research supports the idea that students and technicians who learn to check, check again, and keep reference sheets nearby generate less chemical waste (Jones et al., 2021, Journal of Chemical Education). These habits don’t just save on raw materials—they keep unnecessary toxics out of drains and dumps. With 4-Bromofluorobenzene, that’s no joke. Bromine products cost extra to dispose of safely.
Beyond the Number: Safety and Regulation
4-Bromofluorobenzene isn’t harmless. Both brominated and fluorinated rings participate in reactions that produce persistent organic pollutants. If you trust your math, you cut down on spills and avoid over-preparation. Following safety data sheets from the start, thanks to knowing just how many grams you’re working with, locks in safer habits. Overshooting on stock solutions ramps up fume hood exposure and bumps up the price tag during hazardous waste collection. Each gram adds up in real-world budgeting.
Regulations tie into purity standards, too. Chemical suppliers check incoming batches for impurities by calculating what should be present, confirmed by mass spectrometry. If the molecular weight is off, red flags go up. The US Environmental Protection Agency and its European counterparts care deeply, since errors can reach downstream products that people and wildlife encounter. No competent lab shrugs off numbers like this.
How to Keep It Straight
My old trick: tape up flawless reference charts next to the balance, no matter how good you think your memory is. In high-throughput labs, shared digital calculators and regular training catch most mistakes before they cause financial pain. Open databases like PubChem and Sigma-Aldrich also put accurate data a click away. Routine drills—think mock-weighing with colored sand—help new lab techs get confident. Small steps like these help teams avoid chemical blunders, environmental headaches, and legal battles over contaminated batches.
Getting the molecular weight of 4-Bromofluorobenzene right isn’t about academic pride. It’s about accountability, lab safety, and saving everyone’s time on the job.
Science sometimes sounds a lot fancier than it is. Working with chemistry in the lab, I learned really fast that numbers like “boiling point” matter way more than you’d think. For students and folks in research, 4-Bromofluorobenzene comes up in organic chemistry labs. Its boiling point isn’t just a number in a textbook. It’s about how safely you can distill it, keep it stable, and even how you store it.
Why Boiling Point Matters More Than Most Admit
4-Bromofluorobenzene is a mouthful, but in practice, I’ve found it’s easier to remember what happens to it over a flame or a hot plate. Most standard references put its boiling point right around 152 degrees Celsius. You’ll notice, if you ask two instructors, sometimes you’ll get numbers within a degree of that mark. That’s from the way labs measure, sometimes varying humidity, or even old thermometers. But compared to water’s 100 degrees Celsius, you can see right away this stuff is a bit more stubborn to vaporize.
The point isn’t to just check a safety box. Boiling point drives so many decisions. Say your project involves separating a mix of compounds: you have to choose solvents or design your setup so that nothing decomposes or explodes. Get the boiling point wrong, you risk inhaling toxic fumes or wasting hours on a distillation gone sideways. For someone who once sang eyebrows off with a careless reflux, the right data saves real pain.
Understanding Chemical Safety and Storage
Chemicals like 4-Bromofluorobenzene turn up in research and industry settings. I’ve seen storage nightmares—bottles sweating in hot rooms, ventilation on the fritz. If you forget that boiling point hits well above most summer afternoons, you run less risk with 4-Bromofluorobenzene compared to more volatile substances. Still, labs never relax. Fume hoods and safety goggles go on, and personnel get briefed, because fumes and spills always sneak up.
Research shows that handling aromatic halogenated compounds safely reduces long-term health issues in lab workers. An American Chemical Society report tracked exposure-related problems years after researchers left poorly ventilated environments. That drives home why knowing the boiling point isn’t trivia. It’s part of keeping people healthy and workspaces safe, especially since similar compounds (like bromo- or chlorobenzenes) each come with separate sets of hazards.
Better Practice, Smarter Solutions
I’ve worked with professors who keep laminated sheets—facts like boiling points, melting points, flash points—next to the fume hoods. More labs could use that. Instead of relying on memory or slow searches, reference info is right where you need it. Digital tools bring this idea into everyday practice. Mobile apps with searchable chemical databases help students instantly find figures and safety protocols.
Study after study finds that chemical accidents drop when teams review boiling points and similar metrics before starting. No one likes cleanup crews, paperwork, or the aftertaste of burnt eyebrows. Simple habits—annotating notes with correct figures, reviewing materials as a team—reduce mistakes and protect everyone’s breathing space.
The story of 4-Bromofluorobenzene’s boiling point proves that science is practical. Get the facts, use them, and work safer. It’s just good chemistry.
| Names | |
| Preferred IUPAC name | 1-Bromo-4-fluorobenzene |
| Other names |
p-Bromofluorobenzene
1-Bromo-4-fluorobenzene 4-Fluorobromobenzene p-Fluorobromobenzene |
| Pronunciation | /ˈbrəʊ.moʊˌfluː.əˈbɛn.ziːn/ |
| Identifiers | |
| CAS Number | 460-00-4 |
| 3D model (JSmol) | `3D model (JSmol)` string for **4-Bromofluorobenzene**: ``` CCCC1=CC=C(F)C=C1Br ``` (Note: This is a SMILES string representation suitable for most 3D molecular viewers, including JSmol.) |
| Beilstein Reference | 1209220 |
| ChEBI | CHEBI:36960 |
| ChEMBL | CHEMBL51793 |
| ChemSpider | 85705 |
| DrugBank | DB14171 |
| ECHA InfoCard | 100.017.859 |
| EC Number | 205-622-1 |
| Gmelin Reference | 80847 |
| KEGG | C19741 |
| MeSH | D015745 |
| PubChem CID | 69707 |
| RTECS number | CU9100000 |
| UNII | LT2K5R5FSW |
| UN number | NA1993 |
| Properties | |
| Chemical formula | C6H4BrF |
| Molar mass | 175.01 g/mol |
| Appearance | Colorless liquid |
| Odor | Aromatic |
| Density | 1.473 g/mL at 25 °C (lit.) |
| Solubility in water | Insoluble |
| log P | 3.7 |
| Vapor pressure | 2.7 mmHg (20°C) |
| Acidity (pKa) | 43.7 |
| Basicity (pKb) | 15.55 |
| Magnetic susceptibility (χ) | -76.0e-6 cm³/mol |
| Refractive index (nD) | 1.5000 |
| Viscosity | 0.823 cP (20°C) |
| Dipole moment | 2.60 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 325.5 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | −57.7 kJ mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -4160 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H302: Harmful if swallowed. H315: Causes skin irritation. H319: Causes serious eye irritation. H335: May cause respiratory irritation. |
| Precautionary statements | P210, P233, P240, P241, P242, P243, P261, P264, P271, P280, P301+P310, P303+P361+P353, P304+P340, P312, P330, P370+P378, P403+P235, P405, P501 |
| NFPA 704 (fire diamond) | 2-2-0 |
| Flash point | 51 °C |
| Lethal dose or concentration | LD50 Oral rat = 3060 mg/kg |
| LD50 (median dose) | LD50 (median dose): 2000 mg/kg (rat, oral) |
| NIOSH | RN1055 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.1 ppm |
| IDLH (Immediate danger) | Not established |
| Related compounds | |
| Related compounds |
Bromobenzene
Chlorobenzene 4-Bromotoluene Fluorobenzene Iodobenzene Nitrobenzene |
