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Chemistry doesn’t always get the spotlight, but 4-bromoaniline has quietly supported advances in research, medicine, and industry for well over a century. This aromatic amine pops up in classic texts on synthetic dyes and pharmaceutical building blocks. Early chemists, often working with few resources, discovered the value of brominated anilines as they searched for new ways to modify the color and durability of synthetic dyes. By the late 1800s, these compounds earned a spot in catalogues that would lay groundwork for textile colorants and reagents. In my experience leafing through old case studies and German chemistry journals, I’ve seen how brominated aromatics like 4-bromoaniline transitioned from bench curiosities to serious ingredients supporting larger chemical research endeavors. Their clear synthesis routes meant students and innovators could learn practical organic skills without too many detours.
Today, 4-bromoaniline shows up most often as a white to pale tan crystalline powder, with a mild, sometimes pungent odor. It’s one of those chemicals you find not just on shelves in research labs, but in industrial storerooms tucked between more prominent chemical compounds. Its value doesn’t come from dazzling properties alone; it lies in its flexibility as a building block, used mostly by people aiming to make something even more complex. From the synthesis of fine chemicals to specialized pharmaceuticals, the compound’s presence runs deeper than most outsiders realize. Over the years, smaller companies and university labs have relied on 4-bromoaniline as part of routines designed to teach practical synthesis, purity determination, and advanced organic modifications.
4-bromoaniline features a benzene ring attached to an amino group and a bromine atom—positions separated at the “para” slots. Its molecular formula is C6H6BrN, and it tips the scales at just over 172 grams per mole. Melting point hovers close to 66-67°C, with a boiling point around 270°C. I’ve noticed that cautious handling remains a norm in teaching labs: the material won’t combust at low temperatures but doesn’t play well with open flames or mixing with strong oxidizing agents. Its solubility skews towards organic solvents like ethanol and ether more than water, making purification and isolation relatively simple during small-scale synthesis routines. I still recall the first time isolating this compound in a student lab—white, sharp-edged crystals filtering out of solution, a clear sign of textbook recrystallization in action. Review articles describe its chemical stability as moderate; it’s sensitive to prolonged exposure to strong acids but stands up reasonably to most lab conditions.
Clarity and accuracy on labeling drive safety and efficiency with chemicals like 4-bromoaniline. Most suppliers use standardized GHS (Globally Harmonized System) pictograms—highlighting both its toxicity and environmental risks. You’ll normally see CAS number 106-40-1 on bottles. Purity levels range from the typical 98 percent on research-grade packages, to slightly lower values for industrial scaling. Lot codes, batch tracking, and expiry dates support traceability and regulatory compliance. In older stockrooms, I’ve seen faded, handwritten tags—today, strict technical documentation leaves less room for error. These evolving labeling practices help keep labs and storage areas safer, reducing chances for mix-ups or mishandling in high-pressure settings.
The bread-and-butter approach to making 4-bromoaniline starts with nitration of bromobenzene followed by reduction, but many labs choose to start with the bromination of aniline itself, using bromine or N-bromosuccinimide, under controlled temperatures. In textbooks, you’ll read about fume hoods, ice baths, and careful addition; as someone who has guided students through the process, I can vouch for the value of ingraining methodical habits. Key is controlling reaction temperature and using adequate ventilation—the fumes can sting unprepared noses. Scale affects difficulty: a gram-scale prep in a teaching lab runs smoothly with routine safety equipment, but scaling up in an industrial plant shifts attention to efficient mixing, heat transfer, and containment. Green chemistry pushes toward procedures that cut out harsh reagents or minimize hazardous waste, shifting more labs toward catalytic bromination or modern photochemical methods.
In synthetic laboratories, 4-bromoaniline doesn’t stand still. It’s a launchpad for further chemical modification—whether via nucleophilic substitution, palladium-catalyzed cross-coupling (think Suzuki-Miyaura and Buchwald–Hartwig amination), or forming diazonium salts for subsequent transformations. Recent papers focus on how the para-bromine group allows for selective substitutions, letting chemists introduce a wide range of functional groups under relatively mild conditions. I’ve seen it play a key role in pilot projects where the end goal is a tailor-made pharmaceutical intermediate, dye, or agrochemical. The amino group often finds itself protected or acetylated before further modification, keeping yields robust and undesired side reactions minimal. This versatility keeps it popular in both academic and industrial circles.
No shortage of names here: 1-bromo-4-aminobenzene, p-bromoaniline, and para-bromoaniline all refer to the same compound. On chemical inventories or Safety Data Sheets, you might also run across less common designations like 4-bromophenylamine. I’ve found it useful to double-check sample IDs, since confusion sometimes creeps in when older lab notebooks and digital catalogs use different naming conventions. Academic teams tend to standardize around IUPAC naming these days, but the synonyms sometimes persist on packaging and invoices, slowing down audits or data cross-checks.
Risks run higher than with table salt or aspirin—direct skin contact can cause irritation, and inhalation leads to respiratory discomfort. Chronic exposure links to nervous system symptoms, so most workplaces set up designated fume hoods, gloves, and splash-resistant eyewear. Chemical hygiene officers repeatedly mention the importance of routine leak checks and ventilation system upkeep. Spill cleanup trainings emphasize the value of fast action, and post-use storage in tight-sealing containers away from strong oxidizers. In regulated industries, exposure monitoring and proper disposal keep staff and the surrounding community safer. I’ve worked in both under-funded university teaching labs and large-scale pilot plants; regardless of budget, sticking to a detailed safety routine pays off every time.
4-bromoaniline finds its way into pharmaceuticals, agricultural chemicals, and in the synthesis of specialty dyes and pigments. Drug designers exploit its ability to serve as an intermediate—building key structures for antihistamines and antimalarials among others. In textile chemistry, research keeps popping up about its use in the creation of azo dyes and more stable colorants for synthetic fibers. Over the past two decades, custom electronic materials and polymers have begun calling on brominated anilines to improve conductivity or thermal resistance. The diversity of its application grows with every innovation in synthetic organic chemistry—the more ways chemists learn to modify aromatic compounds, the broader 4-bromoaniline’s utility becomes.
Much of the recent R&D effort revolves around sustainable production and conversions that minimize environmental impact. Academic groups focus on green chemistry routes—using enzymes, milder brominating agents, or flow chemistry to cut down on hazardous byproducts. In industrial labs, teams experiment with automation and in-line monitoring to boost yield and purity, supporting both pharmaceutical quality standards and tighter environmental regulations. Ongoing improvements to analytical methods—like real-time NMR and chromatography—help scientists better track impurities and reaction progress, reducing waste and improving product safety.
Toxicological studies report that 4-bromoaniline carries risks even at low levels of chronic exposure, especially through inhalation and skin absorption. Animal testing links long-term contact to methemoglobinemia, a blood disorder, along with possible nerve and organ effects. Regulatory bodies in North America, Europe, and Asia require rigorous environmental and biological handling guidance for industrial users. Lab protocols stress minimizing airborne powders, immediate decontamination after spills, and never eating or drinking near active experiment sites. Companies developing large-scale processes must invest in staff training, full safety documentation, and medical monitoring where prolonged exposure might occur.
Looking forward, demand for specialty amine intermediates continues to climb, spurred by emerging pharmaceuticals and custom materials. As the push for greener and safer chemistry grows stronger, I expect further breakthroughs in catalytic bromination and safer alternatives for synthesis. Collaborations between academia and industry often speed these transitions, with new methods trickling down from publication to plant floor in just a few years. Data-driven process optimization, using machine learning to predict impurity formation or select ideal reaction conditions, is likely to transform how future generations of chemists produce and use 4-bromoaniline. With careful balancing of innovation and safety, this “quiet workhorse” will keep underpinning chemical progress in fields as varied as healthcare, electronics, and advanced manufacturing.
4-Bromoaniline stands as a chemical with real value in dye synthesis, pharmaceuticals, and even daily product development. Its structure and formula form the backbone of many modern applications. The molecular formula for 4-Bromoaniline is C6H6BrN. In simple terms, it features a benzene ring with an amino group (-NH2) attached to the first carbon and a bromine atom sitting at the fourth carbon—that’s why it’s called para-bromoaniline. The systematic name, 4-bromobenzenamine, reflects this arrangement. A skeletal formula would show the bromine and amino groups sitting across from each other on the ring.
Anyone who has spent time in a lab knows this kind of molecule isn’t just an academic exercise. The presence of both an electron-donating group (amino) and an electron-withdrawing group (bromine) on the benzene ring creates a set of properties that chemists tune for specific results. This combination shapes everything from reactivity in classic electrophilic substitution reactions to the way the compound gets processed by enzymes in biology. The arrangement, while simple, gives direct routes for further substitutions or coupling reactions. That’s why chemists reach for it when crafting new molecules for dyes, pesticides, or drugs.
Ignoring structure leads to missed opportunities. For 4-Bromoaniline, the formula C6H6BrN doesn’t just represent a sum of elements. It tells researchers a lot about its potential uses and risks. For instance, the bromine atom sitting at the para position means the molecule can undergo specific reactions that create azo dyes—these show up on everything from sports jerseys to hair colorant. The amino group acts as a key site in pharmaceutical chemistry, supporting transformations that create more complex active compounds. Knowing these groups’ positions makes a world of difference during synthesis. Casual mistakes in positional isomerism could mean ending up with a substance that’s useless or even harmful.
Anyone working with chemicals like 4-Bromoaniline carries a responsibility. The compound has demonstrated toxicity in laboratory studies, affecting both aquatic life and human health if ignored. Chemical structure guides safe handling protocols. The bromine group makes the compound more reactive, requiring solid protective measures—goggles, gloves, and fume hoods aren’t optional when working at the bench. In the past, lapses in attention around aromatic amines have led to workplace illnesses. I remember a story from my studies where improper ventilation forced a shutdown of an otherwise productive lab for weeks.
Clear labeling, updated training, and regular safety audits trump wishful thinking. Sharing data openly in chemistry communities means fewer accidents and better results. Organizations like the American Chemical Society publish regular guides and safety updates based on cases involving compounds like 4-Bromoaniline. Researchers now track the environmental impact of these molecules, making moves toward greener, less hazardous alternatives where possible. Substituting halogenated compounds with less persistent chemicals marks progress, but informed choices mean everything—structural knowledge always leads those decisions.
While the formula C6H6BrN captures the technical detail, understanding the shape, orientation, and history of its use brings richer insight. Chemistry remains a field grounded in facts, but its real progress depends on those who engage with these molecules, understand the risks, and work toward better solutions for users and the environment alike.
4-Bromoaniline stands out in chemistry circles for its unique structure—a benzene ring with an amine group and a bromine atom. It’s a starting point for a range of reactions and serves as a bridge to more complicated molecules. I remember my early days in an organic chemistry lab, and compounds like this were always on the shelf, ready to spark a new idea or keep a reaction moving forward. Its uses reach into industries that shape our everyday lives.
Many pharmaceutical products rely on variations of aniline as building blocks. 4-Bromoaniline feeds directly into this process. Medicinal chemists use it to create key intermediates for antipyretics, anti-inflammatory drugs, or even treatments for psychiatric conditions. The presence of bromine at the fourth position gives chemists more flexibility, paving the way for producing molecules that can target disease with precision. For example, brominated anilines launched the development of important medications, aiding efforts to fight cancer or bacterial infections. People often don’t see the link between lab chemicals and lifesaving drugs, but it’s there at the foundation of many medicines.
Out in the field, 4-Bromoaniline finds a use in the creation of herbicides and fungicides. Some of the most effective plant protection products on the market begin with aniline derivatives. By making these compounds, chemists can respond to emerging threats to the food chain, pressing back against crop diseases and invasive weeds. Production of agrochemicals based on 4-Bromoaniline means farmers can prevent losses, keep up with demand, and reduce waste in the supply chain. This translates to more reliable grocery shelves and affordable food for families.
Many of us encounter 4-Bromoaniline without noticing, in the form of color on clothing, inks, and plastics. The chemical acts as a precursor in dye production. Textile labs mix it into reactions that yield vivid hues and stable pigments. Thanks to this compound, designers can create colors that last through repeated washes and wear. Its role in producing specialty dyes lets consumer goods stand out—think of a bright shirt that stays eye-catching after months of use. Factories rely on this stability to reduce excess waste from faded or unsellable product lines.
Academic and industrial labs return to 4-Bromoaniline time and again for custom synthesis projects. Its functional groups make it a useful tool for exploring new reactions. My colleagues and I once explored its potential in creating sensor materials and advanced polymers. Researchers depend on its reactivity—using it in Suzuki or Buchwald-Hartwig reactions, for example—to piece together novel molecules that could one day fuel everything from electronics to environmental sensors.
Handling 4-Bromoaniline takes care. Exposure can irritate skin or eyes, and long-term risks need attention. Factories must use protective equipment and follow waste treatment protocols to keep people and the environment safe. Companies adopting green chemistry approaches can limit dangerous byproducts and work toward processes that waste less and pollute less. Investing in better containment, recycling solvents, and reducing exposure helps chemical plants remain compliant with regulations while protecting the workforce. People involved—from researchers to factory staff—deserve safe conditions as much as consumers deserve products they can trust.
Working with chemicals in any setting calls for respect—4-Bromoaniline especially deserves that kind of attention. This compound, used in dye manufacturing and pharmaceutical research, doesn’t telegraph its risks with a bright warning sign, but the dangers are real all the same.
Accidental exposure is more common than most hope, especially if lab routines get sloppy. 4-Bromoaniline can irritate skin and eyes after even brief contact. You could brush against it by accident and find a red patch spreading before lunch. If it gets in your eyes, expect burning and lasting discomfort. Micro-particles sometimes float up as dust during weighing or transfer; inhaling them may cause sore throat, coughing, or nausea. People who don’t wear gloves or goggles—maybe thinking it’s just another day in the lab—might realize too late that direct contact often brings trouble.
Swallowing 4-Bromoaniline, which can happen through contaminated hands or surfaces, brings up serious concerns. Nausea, dizziness, and even blue-tinged fingers (a sign your body isn’t getting enough oxygen) become possible. It’s not scare talk—it reflects real cases reported in occupational health records. This compound affects how the body processes oxygen, so even less-than-obvious exposures stack up over time.
For those working with this compound, gloves, splash-proof goggles, and lab coats almost become a second skin. Ventilation matters too: fume hoods or well-placed exhaust fans help keep airborne bits from invading lungs. Sometimes small labs skip this step to save time or space, but cutting corners there rarely ends well. After long days in the lab, I find it’s best to treat every cleanup as seriously as the experiment, since dust and liquid residues both linger in unexpected places.
4-Bromoaniline needs to stay away from heat and open flames. It’s not the most flammable compound, but why tempt fate? Locked cabinets, clear labels, and dry environments help avoid unwanted reactions. Spills happen, especially during transfer between containers. I keep spill kits stuffed with absorbent pads, neutralizing agents, and disposable gloves within arm’s reach, not buried in some supply closet. Having the right gear can turn a crisis moment into just another cleanup.
Regular training pays off. Practical drills help everyone learn what to do if things go sideways: how to use the eye wash, where to find emergency showers, and how to safely bag contaminated materials for disposal. Labs that treat these routines seriously see fewer injuries. It helps when leaders set a clear tone—no one should get hassled for wearing too much protective equipment.
Some companies now substitute 4-Bromoaniline with less hazardous compounds wherever possible. Finding replacements can take effort and money, but fewer health scares make the switch worth it. When substitution isn’t practical, having protocols to limit exposure—shorter work periods, strict hygiene routines, and detailed record-keeping—keeps risk in check.
Talking about safety precautions isn’t just a box-ticking exercise—it's looking out for each other in a space where mistakes can mean harm. A workplace culture that values real safety over speed means less time lost to accidents and a healthier team in the long run.
Anyone who has spent time around chemical labs knows how the little habits of care make a big difference. 4-Bromoaniline serves as a good example. This chemical steps into research, pharmaceutical work, and dye manufacturing. Its health risks call for serious attention, not just routine handling or storage.
A dry, cool, and well-ventilated place protects both the chemical and everyone nearby. Small leaks or careless exposure can irritate the eyes, skin, or respiratory system. Because 4-Bromoaniline can harm organs through repeated or long-term exposure, you want to keep it sealed away in tightly closed containers made out of compatible materials. Glass and certain plastics do the job, while metal sometimes reacts with amines like this one. Every workplace I’ve visited that respects its people and its assets follows this practice with consistency, not only for paperwork but for safety’s sake.
I have seen too many “mystery bottles” on crowded shelves. If a bottle doesn’t carry a clear label with the chemical name, date, and hazard warnings, it’s no better than leaving a loaded trap for someone down the line. Establishing rules for chemical storage often proves more important than the choice of shelving itself. 4-Bromoaniline belongs in a designated area for toxic or harmful substances, locked away from acids, oxidizers, or things like strong bases that might trigger dangerous reactions. Experienced teams will tell you that segregating chemicals cuts down on both near-misses and outright accidents.
In every lab I’ve walked through, the glove box and the face shield are right up front. Nitrile or neoprene gloves stand up to anilines much better than bare skin or thin alternatives. Wearing laboratory coats, safety goggles, and gloves might feel routine, but that habit means no one leaves their shift with stained fingers or irritated eyes. A fume hood always comes into play with 4-Bromoaniline, since inhaling dust or fumes brings on headaches or worse – and the best ventilation systems stay tested, not just installed once and forgotten.
4-Bromoaniline won’t burst into flames with a stray spark, but its organic makeup means fire risk can’t be ignored. Dry chemical extinguishers, CO2, or foam deal with possible fires. Water often spreads chemical spills, so fire marshals prefer to keep water nearby for overall site safety but not for chemical fires. Safety data sheets need an accessible place, not buried in a drawer, so anyone on-site knows the risks and the right first steps if there’s a spill or exposure.
I’ve met old-school chemists who treat training as a living thing, not a once-a-year formality. By keeping staff familiar with both hazards and emergency plans, mistakes become rare. Practicing spill drills or testing fume hoods reminds everyone that safety isn’t just about following rules. It’s a mindset that respects both the science and the people doing it.
Good handling and storage of chemicals like 4-Bromoaniline go beyond catchy slogans. The safest places I’ve worked all have checklists, not just for compliance but to keep risk low and confidence high. Groups that ask questions and encourage double-checking waste less product, reduce health problems, and build trust among their people. That’s the culture every chemical workspace should aim for.
4-Bromoaniline often shows up on order lists for companies making dyes, pharmaceuticals, or specialty polymers. Tools and training aside, success usually starts with the quality of raw materials. Purity in chemistry isn’t a fancy extra—it's core to performance and safety. When I worked in the lab, we tested everything that arrived, because trace contaminants often produced bizarre results or outright failure.
4-Bromoaniline with strong, reliable purity means fewer headaches. If traces of water, metals, or organic by-products sneak in, even on the level of a fraction of a percent, entire batches might show unexpected colors, foul smells, or fail downstream tests. This isn’t just an academic concern. Contamination at the seed stage can cost thousands when scaled up, not to mention regulatory trouble when impurities reach unacceptable levels for finished drugs or food additives.
Buying 4-Bromoaniline involves more than just looking at a white powder in a bottle. Typical chemical supply specifications for this compound list a purity above 99%. The exact assay varies—I've seen lots hover between 99.0% and 99.5% as measured by HPLC or GC. Reputable sources always provide a certificate of analysis. Look for that traceable documentation, not a vague note from the seller.
Other lines on the certificate show numbers for melting point—usually 64–66°C—plus loss on drying and residue on ignition. Loss on drying below 0.5% tells you the powder hasn’t soaked up much water. Low residue on ignition—usually below 0.1%—means inorganic contaminants like silicates and metals haven’t hitched a ride. Each of these might sound technical, but I’ve learned that for process chemists or regulators, every bit assures something hasn’t gone sideways between synthesis and shipping.
Some industries push further, insisting on heavy metal testing or UV/Vis spectrum checks for color stability. Even if you don’t think you need such extremes, the best suppliers publish their data, answer questions, and stay ready to run extra tests for large orders. The extra dialogue shows care and trust in their batch, not just a sales pitch.
In my years of buying chemicals for the bench, we got samples from global and local sources. A label that says “99%” only means something if the lot number matches a real analysis and the supplier responds when you raise a red flag. I’ve experienced contaminated solvents wrecking syntheses, and one time an “off” 4-Bromoaniline produced a shade of dye no client wanted. Tracing the source, we saw that the contaminants matched a fingerprint of the synthetic route used by the manufacturer. Raw materials with the right paperwork still got flagged, saved only by labs that double-check on arrival. Small labs and big plants rarely regret their caution.
Everyone in the chain holds some responsibility. Producers who care about more than volume pay attention to distillation, cooling rates, and even the drums used for shipping. Transparency matters too—publish everything from stability information to recommended storage conditions. Third-party audits and open customer feedback weed out the weak links.
For buyers, never rely on price alone. Demand complete specifications and recent analysis. Send samples for independent checks if something feels off. By focusing on purity, full disclosure, and clear testing data for 4-Bromoaniline, everyone gains—users get peace of mind, manufacturers build a better reputation, and the end products work as intended.
| Names | |
| Preferred IUPAC name | 4-bromoaniline |
| Other names |
p-Bromoaniline 4-Bromo-1-aminobenzene 1-Amino-4-bromobenzene |
| Pronunciation | /ˌbrəʊ.moʊ.əˈnɪl.iːn/ |
| Identifiers | |
| CAS Number | 106-40-1 |
| 3D model (JSmol) | `3D model (JSmol)` string for **4-Bromoaniline**: ``` NC1=CC=C(Br)C=C1 ``` |
| Beilstein Reference | 87424 |
| ChEBI | CHEBI:34619 |
| ChEMBL | CHEMBL15608 |
| ChemSpider | 6829 |
| DrugBank | DB03868 |
| ECHA InfoCard | ECHA InfoCard: 100.004.143 |
| EC Number | 202-155-1 |
| Gmelin Reference | 8227 |
| KEGG | C06585 |
| MeSH | D000780 |
| PubChem CID | 6921 |
| RTECS number | BX0700000 |
| UNII | 7D6E8P478A |
| UN number | UN3447 |
| Properties | |
| Chemical formula | C6H6BrN |
| Molar mass | 172.02 g/mol |
| Appearance | White to beige crystalline powder |
| Odor | Amine-like |
| Density | 1.6 g/cm3 |
| Solubility in water | slightly soluble |
| log P | 1.96 |
| Vapor pressure | 0.00168 mmHg (25°C) |
| Acidity (pKa) | 4.59 |
| Basicity (pKb) | 8.77 |
| Magnetic susceptibility (χ) | -61.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.640 |
| Viscosity | 0.991 cP (20°C) |
| Dipole moment | 2.50 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 122.8 J·K⁻¹·mol⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | 109.3 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -3335.2 kJ/mol |
| Hazards | |
| Main hazards | Harmful if swallowed, causes skin and eye irritation, may cause allergic skin reaction, toxic to aquatic life. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07, GHS05, GHS09 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H332, H341, H351 |
| Precautionary statements | H302 + H312 + H332, H315, H319, H335, P261, P280, P305 + P351 + P338, P304 + P340, P405, P501 |
| NFPA 704 (fire diamond) | 2-2-0 |
| Flash point | 138°C |
| Autoignition temperature | 630°C |
| Lethal dose or concentration | LD50 (oral, rat): 1750 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral-rat LD50: 2700 mg/kg |
| NIOSH | BZ0400000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | REL (Recommended Exposure Limit) for 4-Bromoaniline: "0.5 mg/m3 |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Aniline 2-Bromoaniline 3-Bromoaniline 4-Iodoaniline 4-Chloroaniline 4-Fluoroaniline |
