The road leading to 3-Bromophenol’s modern use stretches back to a period when chemists first tinkered with simple aromatic compounds in hopes of extracting practical value from their structures. Those early years of the organic era, the late 19th century, saw scientists like Friedel, Crafts, and their peers experimenting with halogenations and phenol modifications. As brominating agents found their way into more hands, curiosity about brominated phenols naturally followed. Over the decades, the compound shifted from a topic in academic journals to a familiar presence in chemical catalogs, its uses expanding as research broadened our understanding. Its commercial relevance only began to take shape as industries, ranging from pharmaceuticals to specialty materials, picked up on its versatile structure.
3-Bromophenol stands as one of those aromatic compounds that catches the attention of chemical labs, not because of an explosive popularity, but for the reliable reactivity and accessibility it provides. Obtained primarily through controlled bromination of phenol, its simple structure—essentially a benzene ring with both a hydroxyl and a bromine group—lends itself to many transformations. Many researchers keep a bottle of it ready, knowing it serves as a solid starting point for synthesizing more complex molecules, from agrochemicals to pharmaceuticals. Its commercial form usually appears as crystals or powder, modestly pale and easy to handle, which encourages its use beyond just academic chemistry.
Crystallizing at room temperature, 3-Bromophenol typically appears white or off-white, with a scent sharp enough to stand out—a chemical tang common among phenols but nudged by halogenation. Its molecular formula, C6H5BrO, and a molecular weight near 173.01 g/mol, offer a predictable template for reactivity. Its melting point rests around 32-35 °C, and it boils between 219 and 221 °C under atmospheric pressure. Solubility favors organic solvents such as ethanol, ether, and chloroform, and it barely dissolves in cold water. The presence of both an activating hydroxyl and a deactivating bromine sets up a scenario where substitution reactions need to be chosen with care. Given the bromine atom’s tendency to be a good leaving group, this compound often sees further functionalization or coupling reactions under mild conditions.
Any reputable supplier lists their 3-Bromophenol with a purity percentage, usually above 98%. Labs value accuracy, so certificates of analysis come with each lot—outlining melting point, appearance, and GC-MS or HPLC data to confirm identity. Regulatory compliance is outlined plainly on each label: GHS hazard information, batch number, manufacturer, and recommended storage (cool, dry, out of direct sunlight). Properly labeled bottles help reduce cross-contamination and help comply with OSHA and local chemical safety laws. Anyone working with these bottles in a lab will see pictograms for irritant or health hazard right above the chemical name—the kind of visual cue that shapes safe lab habits every time the vial is handled.
Synthesis tends to follow a straightforward protocol. Most often, chemists dissolve phenol in an organic solvent, then add elemental bromine or a milder brominating agent while keeping the reaction temperature cool. The ortho and para positions relative to the hydroxyl group both present themselves, but with careful control—dilution, temperature, and rate of addition—the monobromo, meta product prevails in good yield. After the reaction completes, water washes remove excess acid and side products, followed by crystallization to purify the compound further. This approach scales quite well, favoring both small-scale lab experiments and batchwise industrial synthesis. The resulting workflow benefits students and workers alike, since even minor deviations help teach fundamental lessons about regiochemistry and reaction kinetics.
The usefulness of 3-Bromophenol branches directly from its dual functional groups. The bromine atom, fixed at the third position, opens the door to Suzuki or Buchwald–Hartwig couplings—a staple in today’s medicinal chemistry for linking complex molecular fragments. On the hydroxyl side, classic ether or ester syntheses lead to libraries of derivatives suited for new materials or pharmaceutical candidates. Electrophilic aromatic substitution, though generally driven by the activating nature of the hydroxyl, takes a new direction due to bromine’s electron-withdrawing pull. Researchers get to experiment with selective reactivity by blocking, deactivating, or tuning these positions, not just to see a reaction run smoother but to uncover unique biological or material properties from subtle modifications.
Ask for 3-Bromophenol at a supplier’s counter, and you might also hear it referred to as m-Bromophenol, meta-Bromophenol, or 3-Hydroxybromobenzene. Each name points to the same ring template with bromine tucked next to the meta spot from the hydroxyl. In catalogs, CAS number 591-20-8 serves as the universal signpost, helping buyers and sellers find precisely what’s required. Some publications might shorten the name to just its initials—BP3—especially when describing screening collections or drug discovery libraries, reminding users that, for all its syntactic variety, the molecule remains the same.
Lab safety officers don’t skip over the safety dossier for 3-Bromophenol. Brominated aromatics demand respect for their irritant and potentially harmful nature. Inhalation or skin contact often leads to irritation, and the fine powder format makes such contact hard to avoid without gloves and fume hood work. Spill protocols and waste handling remain stringent due to both regulatory and environmental risk. GHS hazard statements, including H315 and H319, warn about skin and eye irritation, so even experienced chemists keep goggles, respirators, and spill kits within reach. Material Safety Data Sheets available from suppliers like Sigma-Aldrich or TCI summarize proper handling steps, including ventilation, storage temperature, and emergency procedures. By owning and following these procedures, labs meet both local laws and international standards—no one wants to risk chronic health issues for the sake of a shortcut.
3-Bromophenol’s reach into industry and academia leans far beyond what a first impression suggests. Pharmaceutical research has long used it as a building block for preparing active pharmaceutical ingredients, especially when scaffold diversification is called for in early-stage synthesis. Material scientists use brominated phenols in flame retardants, dyes, and advanced polymers, chasing after new performance metrics or safety standards. In analytical chemistry, it sometimes helps calibrate instruments or works as an indicator in certain titration systems. Even in agriculture, the aromatic template gives rise to herbicidal and fungicidal candidates, though regulatory hurdles limit widespread adoption until safety is proven. As a result, procurement teams in different sectors flag it as a recurring staple, not because it stands alone, but due to its value in forging the next steps of research or development.
Ongoing research always finds ways to turn 3-Bromophenol into a stepping stone for more valuable molecules. The academic journals track modifications, applications in target-oriented synthesis, and use as a probe or intermediate for drug pipelines. In industry, medicinal chemists plot synthetic routes that use its bromine as a functional handle, often as a convergent strategy to speed up SAR (structure-activity relationship) studies. More sustainable synthesis is gaining momentum—the drive for greener bromination avoids harsh reagents, recycles solvents, and minimizes waste. Teams across academic-industry partnerships attempt to engineer biocatalysts or recyclable catalysts, aiming for more selective or low-impact transformations that preserve both cost and environmental standing. Investment in R&D for related phenolic drugs also directs fresh attention its way, bringing in grant money and early-phase clinical interest.
Toxicological understanding of 3-Bromophenol has grown more detailed with the rise of regulatory oversight in the last thirty years. Rodent studies point to moderate oral and dermal toxicity, leading researchers and regulators to recommend strict exposure limits. Chronic exposure carries some evidence of liver or kidney impact, and like other halogenated aromatics, its metabolites sometimes raise red flags for potential bioaccumulation. The compound shows a tendency to irritate respiratory and digestive systems in lab models; this translates into enforceable safety limits in both workplace and environmental contexts. In environmental fate studies, bromophenols display persistence and pose a risk to aquatic life unless efforts are made for proper waste treatment and disposal. Research continues to seek out longer-term ecological impact data, helping lawmakers tune regulatory frameworks and labs design safer substitutes or waste mitigation strategies.
The practical future of 3-Bromophenol intertwines with advances in synthetic methodology, green chemistry, and regulatory compliance. As demand for more efficient drug and material pipelines rises, the utility of this molecule looks set to increase, especially if synthesis becomes greener and safer. Emerging research on sustainable halogenation and downstream modifications opens doors for scaling without magnifying environmental costs. In pharma, the push for faster lead optimization ensures it maintains a place in screening collections and intermediate libraries. Regulatory attention on safety and environmental persistence propels ongoing development of waste treatment systems and safer, biodegradable phenolic alternatives. While new phenolic scaffolds and coupling technologies emerge every year, the adaptability—both chemical and logistical—of 3-Bromophenol continually earns its shelf space in labs and manufacturing lines. Labs and industry outfits keeping an eye on both innovation and responsibility will probably see its footprint remain stable, if not grow, as chemistry takes on new societal challenges.
3-Bromophenol rarely grabs headlines, yet its presence quietly shapes the worlds of research and industry. Walk into a chemistry lab—odds are, bottles with this name sit tucked among far more famous substances. As someone who’s handled more than a few beakers, the sharp, medicinal scent of phenols sticks with me. This tiny molecule means business. So what can it do? Let’s get past the jargon and see why it matters.
Chemists lean on 3-Bromophenol as a building block. It’s no accident, either. With both a bromine atom and a phenol group strapped to a benzene ring, this compound slots into a ton of reactions. Dive into a pharmaceutical lab, and you’ll see it forming the backbone for more complex molecules, some of which lead to antibiotics or anti-inflammatory drugs. I remember mixing up reactions where a single swapped atom flipped an inactive compound to something medical journals would chase. In chemical synthesis, every detail contributes to results, whether you’re crafting a painkiller or a new dye.
Analytical chemistry often gets overlooked—until something catches fire or a batch goes wrong. 3-Bromophenol often helps labs confirm that tests work. Scientists spike their samples with it, and if the machines pick up the spike, results can be trusted. Think of it like adding a bright color to a batch of cookies to spot any missing ingredients. Everyone in the lab breathes easier when they see that signature signal come up, because quality control isn’t just theory; it’s a daily grind.
Step into a distillery, and the tale of 3-Bromophenol takes on a new tone. Distillers and food scientists track its presence in aged spirits and smoked foods, since it’s one of the molecules responsible for earthy, smoky flavors. There’s an art to measuring how much lingers in a bottle of whisk(e)y. Too much, and it tastes off. Too little, and the character falls flat. One small chemical can shift the taste experience, creating the delicate balance found in an aged single malt. As a whisky fan, it’s fascinating to realize that careful chemical monitoring often decides which barrel makes it to a collector’s shelf.
A lot of lab work ends with a trip to the safety binder, especially with aromatic compounds like 3-Bromophenol. It demands respect. Touching or inhaling it risks irritation, and disposal takes planning to avoid environmental harm. My own hands have been stained brown after a carelessly handled phenol—just once. Companies need systems for storage, labelling, and disposal, because a slip can lead to real harm, from researchers’ lungs to groundwater downstream.
Green chemistry points toward using less hazardous substances and recycling chemicals whenever possible. Labs look for cleaner alternatives or ways to reduce the need for special waste treatment. You can’t swap out everything overnight, particularly building blocks as versatile as 3-Bromophenol. Knowledge grows, solutions improve, and with each step, the risks shrink.
3-Bromophenol doesn’t need to trend on social media. Its quiet utility shapes medicine, taste, and technology. Professionals—whether in white coats, work boots, or distiller’s aprons—work every day to keep its benefits high and its hazards low. I’ve learned that the real story in chemistry is never just about a single molecule, but about stewards willing to do the hard, careful work behind the scenes.
Anyone who’s worked in a chemistry lab or just glanced at a bottle of 3-Bromophenol knows the formula doesn’t just help scientists, it shapes how everyday products get made. The chemical formula for 3-Bromophenol is C6H5BrO. This means it’s got six carbon atoms, five hydrogen atoms, one bromine atom, and one oxygen atom. On paper, that looks simple. In reality, the formula also reflects how chemistry touches everything—down to the things used to clean, to test, and to build new medicines.
Back in my student days, learning chemical formulas sometimes felt like rote memorization. Over time, a pattern started to emerge: getting the formula right makes or breaks a reaction. If you’re working on disinfectants, pharmaceuticals, or dyes, the formula is your road map. 3-Bromophenol itself appears as a staple intermediate in organic synthesis. Knowing what those letters and numbers mean isn’t just an academic exercise—it’s what lets researchers explore and create safe products.
It’s not enough to just know that 3-Bromophenol contains bromine attached to the benzene ring at the third position. That subtle shift in position changes how the molecule behaves. Move it to a different spot and you have a new compound, and with that often comes a new set of health and safety data.
A lot of folks working with phenolic compounds grow to respect their risks. Breathing 3-Bromophenol vapors or letting it soak into skin isn’t something you want to experience. Even in well-ventilated labs, that faint medicinal scent is a reminder—handle with gloves, keep it sealed, and don’t take shortcuts. According to the National Center for Biotechnology Information (NCBI), exposure over time could lead to irritation or worse. Guidance from reliable sources, like the NCBI and Safety Data Sheets, proves valuable for anyone regularly handling chemicals like this.
It pops up in lots of research papers for a reason. As a building block, it gives rise to more complex compounds. Sometimes, those products end up in pharmaceuticals, pigments for dyes, or in various industrial processes. The presence of both the bromine and the hydroxyl (OH) functional group means chemists get two reactive sites to work with, giving them flexibility in synthesis.
Companies need to ensure traceability and purity, since impurities could ruin the quality of whatever final product is being manufactured. Rigorous quality controls, regular equipment checks, and precise storage mean fewer accidents and higher trust in research results or finished products.
After seeing the impact of chemical spills and improper disposal, it hardly feels optional to push for better lab management. Waste from compounds like 3-Bromophenol needs careful disposal—never straight down the drain. Local systems can’t always break down industrial chemicals safely. Setting up protocols for waste, automatic containment, and on-site treatment lessens the environmental impact.
Personal accountability ranks up there as well. Sharing knowledge between scientists, consulting updated environmental standards, and promoting continuing education makes a difference. Growing experience points to one truth: paying attention to these details protects people and the planet.
Ask anyone who’s worked in a chemistry lab, and chances are they can recall the biting, chemical tang that comes from using phenol-based compounds. 3-Bromophenol, a colorless to light yellow liquid or solid, carries a strong, medicinal odor that warns you to handle it with caution. Used mostly as an intermediate for dyes and pharmaceuticals, 3-Bromophenol isn’t something most people encounter at home. So what kind of risks do chemists and factory workers face with this chemical?
My time as a chemistry grad student drummed into me that a small tweak in a molecule can change everything. Add a bromine atom to a phenol, and suddenly you’re not just dealing with a sharp-smelling lab reagent — the way your body reacts shifts, too. 3-Bromophenol can cause irritation to the skin, eyes, nose, and throat. Even gloves sometimes feel like flimsy barriers, and that’s a concern. Studies using lab animals have shown that brominated phenols can be absorbed through the skin, which worries health and safety specialists.
Breathing in dust or vapors stings and messes with your lungs. Inhalation in high doses led to coughing, headaches and, in rare cases, more severe central nervous system effects. The U.S. National Institute for Occupational Safety and Health (NIOSH) and European Chemicals Agency both flag 3-Bromophenol for its acute toxicity. It’s not the most toxic thing in a lab, but it’s not something you’d want on your sandwich, either.
Step beyond human health, and 3-Bromophenol raises environmental red flags too. Like a lot of phenolics, it finds its way through wastewater, especially from dye and drug factories. Fish and aquatic critters don’t deal well with brominated compounds. 3-Bromophenol can cause long-term harm to aquatic life at low concentrations. It’s sticky in ecosystems, not breaking down fast, and can move up the food chain.
I remember days in the university lab, double-gloving, using the fume hood, and double-checking the bottle’s cap after use. No one in safety training said the stuff would kill you outright, but all the instructions made its hazards obvious: avoid inhaling the vapor, use splash-proof goggles, wear gloves, and grab a lab coat. The chemical’s safety data sheet makes the point clearer: always use it with good ventilation, never eat or drink around it, and wash affected skin right away.
If a spill happens, sweeping the flakes into a sealed chemical-waste container should be the move. Drain disposal or letting it evaporate is a shortcut that can seep into the water system, and I’ve seen what happens when people cut corners — it’s not pretty.
Better substitution and engineering controls help cut down on exposure. Some labs seek greener alternatives when a safer compound can stand in, but industrial chemistry isn’t always so flexible. Regular air monitoring, improved ventilation, and stricter discharge regulations make a difference. Workers deserve clear information and easy access to protective equipment. From my own experience, I know that regular training works best when everyone knows the “why” behind the safety rules, not just the “how.”
3-Bromophenol demands respect, not just from chemists, but from managers and regulators. This isn’t a household poison, but it’s no joke either. Understanding how it affects your body, your coworkers, and the world outside the factory fence leads to real health and environmental protection.
Working with chemicals always puts a strong emphasis on precision, and calculating the molecular weight isn’t just a chore on a worksheet. Instead, it sets the foundation for just about every lab experiment and industrial process involving that compound. Take 3-Bromophenol as an example. This compound, with a formula of C6H5BrO, shows up in research, analytical labs, and occasionally finds its way as a building block for pharmaceuticals or specialty chemicals.
To figure out the molecular weight, break down the atoms: carbon (C), hydrogen (H), bromine (Br), and oxygen (O). It goes like this—six carbons at 12.01 g/mol each, five hydrogens at about 1.01 g/mol, one bromine at 79.90 g/mol, and one oxygen at 16.00 g/mol. Multiply and add: 6 × 12.01, 5 × 1.01, plus 79.90, plus 16.00. That gives 72.06 (C), 5.05 (H), 79.90 (Br), and 16.00 (O). The sum comes to 172.01 g/mol. Most databases report between 172.01 and 172.02 g/mol, due to rounding, but either figure lands you in the same practical place.
Picking the right molecular weight goes beyond theory. I’ve been in labs where a single calculation slip meant starting an entire synthesis over or misdiagnosing the identity or purity of a sample. Molecular weight figures into stoichiometry, toxicology, and purchasing decisions—every calculation for mixing reagents, scaling up a process, or dosing a substance stems from knowing the exact mass you want. Researchers and students often learn this the hard way the moment a reaction goes sideways due to an overlooked decimal.
Reliable data sources matter as much as a good calculator. Peer-reviewed journals, established chemical suppliers, and standard-setting organizations like IUPAC and NIST all stick closely to reported values. For 3-Bromophenol, things get cross-checked between databases such as PubChem and Sigma-Aldrich. In my own work, a double-check at this stage often saves time down the road. With fake or out-of-date data floating around, dropping in a misspelled name or wrong molecular formula sometimes leads to frustrating and expensive mix-ups.
Laboratory work with 3-Bromophenol often centers on synthesis or analytical reference standards. Chemists and students rely on knowing the precise molecular weight to weigh out just enough substance for a reaction or prepare calibration solutions. Sometimes, this knowledge helps design safer handling and waste protocols—bromine's presence lifts the molecular weight compared to other phenols, which changes toxicity and environmental profiles. Many industrial safety sheets tie risk assessments and necessary personal protection directly to the molecular mass of the substances involved.
Paying attention to calculations might seem tedious, but science relies on tiny details done well. From preparing lab solutions by mass to keeping experiments reproducible, accuracy at this level creates trust in results. Searching for molecular weights in the right places and understanding what separates 3-Bromophenol from its cousins can set apart routine lab runs from real breakthroughs. For anyone working or studying in chemistry, these numbers matter in every bottle, flask, and balance beam.
Anyone who’s worked in a lab for more than a week knows that chemical storage often finds itself at the bottom of a hectic priority list. If you’ve cracked open a bottle of 3-Bromophenol, you’ll remember its sharp, lingering smell and the unmistakable warning labels. You don’t forget how strong this compound can feel on the skin, or how quickly the room air changes after opening a bottle. Storing it safely isn’t just good practice—it helps protect everyone in the room, extends the shelf life of the chemical, and avoids unnecessary headaches for people doing inventory next year.
3-Bromophenol comes as a white to tan solid, and even though it looks pretty tame, it brings risks. This chemical gives off vapors that can irritate your nose, throat, and skin. Too much exposure over time signals real health issues, ranging from breathing problems to skin sensitivity. And let’s not gloss over the fire risk—phenols sometimes surprise folks, especially in older storerooms packed with all kinds of bottles that should’ve been trashed a decade ago.
Personal experience taught me not to trust the back corner of a hot supply closet. Keep 3-Bromophenol in a cool, dry spot, out of direct sunlight. Moisture turns things ugly—lids stick, and you risk unexpected reactions with vapor in the air. I’ve seen too many expensive batches ruined because of a leaky cap or a shelf right above the steam pipes.
The right container matters. Glass is best, with a tight screw cap or specialized phenolic top. No one wants their morning interrupted by a spill in the solvent cabinet. Plastic occasionally works, but only if you're sure it’s compatible. Some labs still use old bottles with questionable seals—saving a dollar now may cost hundreds in cleanup, disposal, or health issues later.
Label everything clearly—names, dates, hazard codes. Even if you think you’re the only one running tests, nobody enjoys guessing games in the middle of a busy workday. Choose a dedicated shelf in the flammable or corrosive storage cabinet, depending on your setup and local rules. Mixing strong acids or bases in the same cabinet only increases risk. After a close call mixing incompatible fumes, I always leave phenols on their own shelf.
Lab ventilation isn’t something you notice until something goes wrong—unexpected fumes spread, and you start coughing across the room. Local exhaust, like a well-maintained fume hood or vented cabinet, can help. If you’re in an older building, I’d suggest double-checking that your air system pulls enough to clear volatile compounds. After all, no one wants to make the evening news for a minor chemical emergency that could have been avoided.
Spill cleanup kits belong within arm’s reach. Ask the people who’ve had to mop up a phenol spill—it’s not pretty, and you don’t want to hunt through closets for supplies during the real thing. Pay attention to the material safety data sheet, especially if new hires or students are working with you. It takes half a minute to share tips on gloves and goggles. The extra care keeps mistakes—and insurance calls—at bay.
Folks often forget that safety practices pass down through trained habits, not memos. Training should include real-life examples. I introduce every new colleague to our chemical storage area, making sure they see where 3-Bromophenol sits, how bottles are labeled, and who to call if there’s a spill. Even experienced chemists find it useful to watch how different labs handle the same material.
Storing 3-Bromophenol the right way avoids mess, protects teams, and keeps the focus on the work—not emergencies. No one wants a hard lesson about flammable phenols in the middle of a busy week. Take storage seriously: it’s the small daily choices that keep the lab running smoothly year after year.
| Names | |
| Preferred IUPAC name | 3-Bromophenol |
| Other names |
m-Bromophenol 3-Hydroxybromobenzene m-Bromohydroxybenzene Phenol, 3-bromo- |
| Pronunciation | /ˈθriː ˈbroʊməˌfiːnɒl/ |
| Identifiers | |
| CAS Number | 591-20-8 |
| Beilstein Reference | 1209221 |
| ChEBI | CHEBI:42060 |
| ChEMBL | CHEMBL1200572 |
| ChemSpider | 7471 |
| DrugBank | DB04251 |
| ECHA InfoCard | 100.011.665 |
| EC Number | 204-622-5 |
| Gmelin Reference | Gmelin 136984 |
| KEGG | C01587 |
| MeSH | D000317 |
| PubChem CID | 69428 |
| RTECS number | BP9625000 |
| UNII | 8719M1S55Z |
| UN number | UN2656 |
| Properties | |
| Chemical formula | C6H5BrO |
| Molar mass | 173.01 g/mol |
| Appearance | White to light tan crystalline solid |
| Odor | Phenolic |
| Density | 1.49 g/cm³ |
| Solubility in water | 4 g/100 mL (20 °C) |
| log P | 1.96 |
| Vapor pressure | 0.04 mmHg (25 °C) |
| Acidity (pKa) | 9.16 |
| Basicity (pKb) | 9.2 |
| Magnetic susceptibility (χ) | -70.0e-6 cm³/mol |
| Refractive index (nD) | 1.574 |
| Viscosity | 0.899 cP (20°C) |
| Dipole moment | 2.62 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 96.3 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -27.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3547.6 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H302, H315, H319, H335 |
| Precautionary statements | Precautionary statements: "P261, P280, P304+P340, P305+P351+P338, P312 |
| NFPA 704 (fire diamond) | 2-2-0 |
| Flash point | 81 °C |
| Autoignition temperature | 300°C |
| Lethal dose or concentration | LD50 oral rat 620 mg/kg |
| LD50 (median dose) | LD50 (median dose) of 3-Bromophenol: "680 mg/kg (Rat, oral) |
| NIOSH | BV8925000 |
| PEL (Permissible) | PEL: Not established |
| REL (Recommended) | Ensure adequate ventilation; avoid inhalation and skin contact |
| Related compounds | |
| Related compounds |
3-Bromophenol hydrochloride 3-Bromophenyl acetate 3-Bromophenol-d4 3-Bromoanisole 3-Bromo-4-methylphenol |
