© 2026 Nanjing Finechem Holdings Co., Ltd,
All Right Reserved
Looking at the long line of alkyl halides, 1-bromohexane steps out thanks to its no-nonsense structure and manageable chain length. Organic chemists in the early twentieth century found their way to this clear liquid by following the footsteps of giants like Victor Grignard, who showed how halogenated hydrocarbons could open doors to new molecules. Laboratories started producing 1-bromohexane as soon as bromoalkanes became staples in synthetic chemistry. Early uses stretched from research benches to industrial preparations, moving from rudimentary apparatus to lined flasks and regulated distillation in just a few decades. At my own university lab, instructors always reminded us that compounds like 1-bromohexane helped lay the foundation for not just experimental protocols but entire swaths of chemical theory regarding nucleophilic substitutions and carbon chain extensions.
As an industrial chemical, 1-bromohexane shows up in an array of processes, bridging the gap between small molecule synthesis and larger-scale manufacturing. This colorless, heavy liquid with a faint, sweet odor finds uses from surfactant manufacture to custom pharmaceuticals, essential for anyone assembling longer hydrocarbon chains or introducing bromo groups for further modification. The commercial market often looks past the simplicity of the molecule, focusing instead on its consistent reactivity and predictability—crucial traits when piecing together complex organic syntheses or seeking intermediates for agricultural chemicals. My own experiences with the compound highlight its reliability, especially during student research where unwanted surprises could derail an entire week’s worth of work.
1-Bromohexane lays claim to a boiling point of about 155°C and a melting point just above -90°C, making it a liquid at room temperature. Its density tips the scale much higher than water, clocking in around 1.17 g/cm³, a feature you can’t miss during phase separations. The molecule resists water but blends easily with organic solvents like ether and chloroform. Having a bromine atom attached to a primary carbon, this compound participates in nucleophilic substitution with more vigor than its secondary or tertiary counterparts. Electrophiles like this often find themselves drawn into textbook substitution or elimination reactions, making them valuable lessons in both theory and practice.
Quality standards in most labs demand a minimum purity of 98 percent for 1-bromohexane, monitored by gas chromatography. Labels mark hazard warnings clearly, not just to satisfy legal requirements but because the dense, relatively slow-evaporating liquid poses real threats if inhaled, ingested, or spilled on skin. Accredited suppliers tend to publish accurate technical sheets listing CAS number 111-25-1, molecular formula C6H13Br, and standard safety icons. From my own perspective, taking labels seriously never feels excessive, as mishandling brominated organics often leads to headaches—literal and otherwise.
Labs and factories generally rely on treating 1-hexanol with hydrobromic acid, sometimes in the presence of sulfuric acid, to achieve efficient conversion. A sharp exotherm and a steady stream of hydrogen bromide fumes signal progress. This straightforward process offers decent yields with minimal by-products, letting chemists access larger amounts without the need for arcane methods or exotic catalysts. Newer techniques sometimes replace liquid acid with triphenylphosphine and bromine, cutting waste and improving selectivity when working on a smaller scale or in research contexts where handling concentrated acids brings unnecessary risks. Drawing from teaching lab experience, running this reaction means managing heat and venting, since the byproducts can fill a room with unpleasant fumes if left unchecked.
With a reactive carbon-bromine bond, 1-bromohexane enters the synthetic game easy and quick. Nucleophiles such as cyanide, amines, or alkoxides attack the electrophilic carbon to forge new carbon–carbon or carbon–heteroatom bonds. Many Grignard reactions depend on reliable bromoalkanes, and 1-bromohexane fits perfectly, offering a straight six-carbon backbone for chain elongation or coupling. This sort of reaction can keep you on your toes—moisture or impure reagents can ruin yields—but the underlying principles carry through decades of empirical practice and modern organic methodologies. Modifying 1-bromohexane usually means swapping out the bromine, a well-trodden path for research projects that need new motifs on a familiar scaffold.
Digging into catalogs and journals uncovers a list of alternate names: hexyl bromide, n-hexyl bromide, 1-Hexyl bromide, and normal bromohexane. Though they describe the same molecule, choosing the right term sometimes reveals the researcher's background—those trained in European curricula often favor “n-hexyl bromide” while American texts tend to use “1-bromohexane.” In practical terms, the variety of names makes careful label reading a habit worth keeping, especially when ordering or inventorying chemicals for a busy lab where mistakes can have bigger consequences than just wasted time or money.
Regulators like OSHA and GHS mark 1-bromohexane as harmful if inhaled or absorbed through the skin. The need for fume hoods, gloves, and eye protection never comes as a surprise—those working with brominated solvents quickly learn the cost of a casual approach. Chronic exposure can lead to liver or neurological issues, making personal protective equipment and regular training part of any chemical handling protocol. In my own early days, running a reflux outside a hood landed me with an unpleasant cough and a firm reminder from the safety officer. Beyond individual measures, clear labeling and accessible Safety Data Sheets stay front-and-center in responsible operations, especially in environments with new students or frequent staff turnover.
Uses for 1-bromohexane stretch far beyond bench-top chemistry. It serves as a handy intermediate for producing surfactants, plasticizers, pharmaceuticals, and agrochemicals. As a model substrate, it helps students and researchers test new synthetic routes or elucidate reaction mechanisms. In industry, its predictable reactions and manageable volatility make it suitable for scaled-up processes, especially where a straight-chain bromoalkane brings just the right mix of reactivity and chain flexibility. I’ve seen custom synthesis outfits keep drums of the compound on hand for needs ranging from fragrance modification to pre-polymer functionalization. Its value flows from reliability—chemists and engineers can count on it to do a specific job without impromptu surprises.
Contemporary investigations keep expanding what’s possible with 1-bromohexane. Green chemistry advocates experiment with alternative brominating agents to cut down on hazardous waste. Catalysis researchers use it to benchmark new metal complexes for carbon–halogen activation. The search for more precise, sustainable, and economical routes leads to research into flow chemistry and microreactor designs, aiming to produce bromoalkanes with better control and fewer emissions. I’ve heard seminar talks on computational modeling of nucleophilic substitution, using 1-bromohexane as the archetypal example for SN2 kinetics across different solvents. These efforts fuel the quest for higher selectivity and gentler conditions—a familiar refrain for anyone who’s ever spent hours cleaning up sticky reaction mixtures.
Toxicologists keep a close eye on brominated organics, monitoring their effects on both lab workers and the environment. Reports suggest that exposure to 1-bromohexane at high levels may impact the nervous system or liver in lab animals. Regulatory bodies respond by setting exposure thresholds and encouraging the use of fume hoods and containment wherever possible. I’ve watched as labs pivot away from brominated solvents whenever alternatives exist, though for some transformations, specific reactivity keeps compounds like 1-bromohexane as fixtures in the supply closet. Mitigating long-term risks depends on good hygiene, proper waste disposal, and regular review of the scientific literature as more evidence emerges.
The role of 1-bromohexane in modern chemistry will keep evolving as industry leans toward safer, greener protocols and tighter regulatory oversight. Alternative synthesis routes, perhaps relying more heavily on enzymatic or less hazardous reagents, are under exploration by academic and industrial researchers alike. For now, though, its knack for clean, straightforward chemistry keeps it relevant in teaching labs, specialty manufacturing, and innovation-driven companies. Advances in purification, recycling, and protective equipment may extend safe use, even as safer alternatives draw attention. Continued research promises to clarify how best to balance operational efficiency and safety—a balance the chemical community pursues with a mix of tradition, skepticism, and practical know-how collected over decades.
Anyone with a background in organic chemistry remembers 1-Bromohexane. It's more than just a name in a textbook. This chemical, with its six-carbon backbone and a bromine atom hanging off the end, shows up as a reliable intermediate in a surprising number of manufacturing and research settings. The stuff itself looks like a colorless, oily liquid, but that bland surface hides a reactive tool.
Lab folks use 1-Bromohexane as a jump-off point for making other molecules. It stands as a textbook example of an alkyl halide. You can swap out that bromine atom easily for other functional groups—amines, alcohols, thiols—so it's a favorite for producing custom molecules in the pharmaceutical and agrochemical sectors. Think of it as a set of LEGO bricks with a handy snap-off section.
Researchers reach for 1-Bromohexane in the lab when plotting out a synthetic route. You need something simple that lets you tack on a hexyl chain? This is where you grab a bottle. It enables the creation of a whole family of compounds, including surfactants and plasticizers. Those products end up in cleaning solutions, coatings, lubricants, and even cosmetics.
The pharmaceutical industry leans on compounds like 1-Bromohexane to link together more complex drug molecules. That simple bromine makes it possible to create precise changes in structure without bringing in unnecessary baggage. The importance isn’t in the flash—it's in the reliability. Efficient syntheses save companies millions, and this intermediate keeps that pipeline moving.
People don't always appreciate that training matters just as much as scalability. Chemistry students get a taste of real-world techniques by working with basic alkyl bromides like this one. Those reactions—foundational as they might seem—show up in the textbooks and on the test bench. There’s no better way to learn nucleophilic substitution or understand what a real industrial process looks like than handling actual reagents.
1-Bromohexane poses challenges. If you've ever handled it, you know the warnings: toxic by inhalation, bad for the skin, and a spill is a headache for both the lab and the planet. It’s not the sort of thing you pour down the drain or leave uncapped. Responsible use means proper ventilation, disposal through hazardous waste procedures, and a real respect for personal protective equipment. Environmental risk comes from accidental release and long-term persistence, so manufacturers and research groups invest in containment and treatment.
Science keeps pushing for replacements that hit the same marks without bringing the same baggage. Greener, safer reagents can often serve a similar purpose, but not every process has a simple swap. As chemists learn more, they find routes that cut out toxic intermediates or use catalysts that reduce waste. None of these changes come easy or cheap, but the push comes from real-world necessity. Companies who want to lead—those that care about both safety and innovation—put in the effort because the long-term payoff stands out.
Getting a handle on something as specific as 1-Bromohexane teaches a wider lesson. In the world of chemistry, small changes at the molecular level create visible, practical results. For everyone—whether working in a plant, at a university, or in a regulatory office—understanding what makes a compound useful, risky, or avoidable shapes how we build tomorrow’s solutions.
Everyday life carries a little bit of chemistry in all corners, from the gasoline fueling a car to the simple medicines we keep in the cabinet. Chances are, you’ve never thought much about something as specific as 1-Bromohexane unless it’s been for school or work. Still, knowing what makes up a compound can carry weight. People depend on facts, not just for trivia night, but to make decisions in industry, medicine, and safety. 1-Bromohexane’s molecular formula comes up in labs, chemical supply orders, and safety protocols. No one wants mistakes in any of those places.
1-Bromohexane hints at its own structure in its name. Chemistry naming follows rules as picky as English spelling, and each piece means something. “Hexane” tells you the backbone is a straight chain of six carbons, all linked with single bonds. “Bromo” signals a bromine atom attached somewhere on that chain. “1-” just shows where the bromine lands—on the first carbon of the chain, not lost in the middle somewhere.
To get the formula, break it down. Ordinary hexane has six carbons (C) and fourteen hydrogens (H); that much comes from basic alkanes. Swap out a hydrogen for a bromine (Br), since that’s what “bromo” means in this context. The formula is C6H13Br.
It looks straightforward, but this step matters. A single extra hydrogen or a misplaced halogen changes properties. In the world of pharmaceuticals or industrial coatings, such mistakes mean the difference between a safe product and a regulatory violation.
Lab mistakes cost money, time, and sometimes more. Inaccurate formulas or labels sometimes end up causing dangerous reactions or failed processes. 1-Bromohexane doesn’t sound like a hazardous substance to most, but like many alkyl halides, it’s flammable and not healthy to inhale. Anyone dealing with it, whether in a research lab or a manufacturing plant, expects the label to match the contents. Fact-checking at the formula level anchors safety and technique.
C6H13Br speaks more than just chemical composition. This single molecule shows up as a building block in organic synthesis, helping researchers and innovators sketch out complex molecules step by step. In drug discovery, that chain can turn into something that treats disease. In materials science, small changes give us coatings or fuels with better traits. A strong foundation here powers advances elsewhere.
The world runs better when facts are clear, and chemistry often brings out the best and worst of that need. I’ve seen good research derailed by a bad chemical batch or a wrong assumption about purity. People expect scientists and manufacturers to know their ingredients down to the single atom. Listing the formula clearly, reviewing it for accuracy, and making sure everyone along the chain—from student to industrial chemist—understands what it means all help maintain that trust.
Mistakes with formulas often come from rushed work, poor quality checks, or second-hand sources. Setting up clear double-check systems, using reliable suppliers, and regular staff training cut down on these errors. Many companies now rely on software to cross-check formulas before purchase or production—these tools work only as well as the people using them. Good habits, like writing out structures or formulas by hand and talking through synthesis steps, catch errors before something leaves the lab or warehouse.
1-Bromohexane isn’t a household name, but go behind the scenes in chemistry labs and you find it all the time. This clear, oily liquid sits on shelves where chemists make organic compounds or study reactions. If you work in academia, pharmaceuticals, or chemical manufacturing, odds are you’ve come across a bottle or two.
To people who haven’t faced chemical exposure up close, 1-Bromohexane might look harmless. It barely smells and doesn’t stain your hands right away. But that’s not enough to declare it safe. The compound can seep quietly into the skin, travel through the air as vapor, or sting your eyes if you’re not careful.
Official data from environmental health agencies shows 1-Bromohexane earns its hazard labels for good reason. The liquid irritates skin and eyes. Prolonged inhalation leads to dizziness, headaches, and even nausea. Touching it repeatedly without gloves creates risks, especially if cuts or broken skin let more through. Long-term lab work with this type of chemical, especially if you skip proper ventilation or gloves, can leave your body paying the price.
Take a hard look at toxicity data and you’ll see the danger isn’t just skin-deep. Studies on animals reveal that ingestion or repeated heavy exposure leads to nerve damage, liver problems, and harm to reproductive health. Some researchers compare its action to that of better-known toxins in the brominated hydrocarbon family, molecules with a history of causing trouble for nerves and brain tissue.
I’ve watched colleagues rush to the eyewash station after a single careless splash. The burning and redness are warnings you shouldn’t ignore. Feeling woozy in a poorly ventilated room, stumbling over words, or dealing with a splitting headache—these experiences underscore why protective gear isn’t just red tape. Once symptoms kick in, the stress and uncertainty stick with you long after the bottle’s back on the shelf.
It’s not just workers standing over a fume hood who need to pay attention. Accidental spills or leaks can seep into water, risking harm to aquatic life. Without careful waste handling, contamination stretches out past the lab. 1-Bromohexane is slow to break down in the environment, so what leaves the building may show up in groundwater years later.
A story from a local research facility brought that risk home for me. After a poorly contained spill, the cleanup teams spent weeks tracing possible leaks and testing soil for contaminants. Add the cost of damage control to the worry for neighbors living downstream, and the message gets sharper—chemical safety isn’t just an indoor problem.
Working around 1-Bromohexane demands a good memory and respect for safety training. Gloves and goggles belong on everyone in the room. Ventilation keeps invisible fumes from building up, and clear protocols for spills make a world of difference. Every new technician I’ve taught gets the same advice—assume every bottle could bite back.
On a bigger scale, industries that use large amounts of this solvent need to invest in waste containment. Dedicated disposal routes, regular environmental testing, and switching to greener alternatives when possible—these actions leave a longer-lasting impact than any warning label. Holding people and organizations accountable for safe practices turns this once-invisible threat into something manageable and respected.
As long as 1-Bromohexane remains in use, clear communication and action on safety matter. Take the science seriously, listen to those who’ve made mistakes, and remember that true expertise means protecting people both inside and outside the lab.
1-Bromohexane, a colorless liquid with a strong odor, has found a place in labs and chemical manufacturing. It’s used in organic synthesis, which makes it a key tool for chemists. With a boiling point around 155°C and moderate volatility, it doesn’t demand cryogenic care but isn’t a low-risk substance either.
Spending time around chemicals like 1-Bromohexane has taught me caution. It’s not just about the label on the bottle—the risks get personal if ignored. 1-Bromohexane irritates the eyes, skin, and lungs. In spaces without proper ventilation, its vapor can build up quickly. Safety Data Sheets point out that repeated or prolonged exposure leads to more than short-term discomfort, possibly triggering nervous system symptoms.
Chemicals last longer and cause fewer accidents when they stay away from direct sunlight and high heat. 1-Bromohexane turns unstable if exposed to temperatures above its boiling point or if mixed with strong oxidizing agents. In my own lab, I’ve seen what happens when a bottle is accidentally left near a window—yellowing liquid, cracked seals, and a growing stink—proof that light and heat speed up chemical breakdown.
It’s tempting to pour chemicals into any empty bottle, but that’s a shortcut with big risks. Strong glass vials with screw caps keep vapors contained better than plastic. Polyethylene plastics hold up against most chemicals, but glass resists reaction the longest. Clear labeling—name, concentration, and hazard symbols—makes a huge difference. I’ve learned from colleagues’ mistakes that one unlabeled beaker is all it takes to turn a safe shelf into a hazard zone.
Any flammable chemical belongs in a flame-resistant cabinet. 1-Bromohexane doesn’t combust easily at room temperature, but its vapors linger close to the ground and can ignite if an open flame appears. Lab rules call for storage below eye level—fewer knocks and drops, and less risk of splashes if a bottle breaks. Flammable liquid cabinets should stay cool, dry, and far from busy walkways to lessen accident chances.
Nobody expects leaks, but ignoring a small drip on a bottle is an invitation for trouble. All it takes is a damp paper towel, and pretty soon that surface is slick and the air feels strange. Any spill should go straight into a sealed hazardous waste container, never down the drain. Spill kits with absorbent pads and gloves should always sit nearby—waiting to hunt for cleanup gear wastes precious seconds.
Even storage plans fall apart if the team doesn’t pay attention. In workplaces I trust, staff run through regular chemical safety drills, check expiration dates, and keep an eye out for decimal point errors in labels or logging. Good records turn everyday handling into a routine instead of a guessing game.
Storing 1-Bromohexane isn’t about fancy systems. It boils down to respecting health risks, choosing solid containers, and placing chemicals somewhere cool, dry, and dim. Regular practice, not just theory, makes sure safety becomes habit. These steps might seem simple, but they protect both people and the work they care about.
I’ve come across 1-Bromohexane in both classroom and practical settings, running distillations and setting up straightforward nucleophilic substitution reactions. This compound carries a simple structure: a six-carbon alkyl chain with a bromine atom fastened to one end. At first glance, it looks like just another organic liquid. Get it on your skin, though, and the faintly sweet, chemical-like odor hangs around—hard to forget after handling it during an undergraduate synthesis.
1-Bromohexane is a clear, colorless to pale-yellow liquid. If you tip a vial of it, the liquid runs a little slower than water. That’s the higher density in play, close to 1.18 grams per milliliter. In hands-on work, this means it sinks if it finds its way into a water bath. The density owes a lot to the heavy bromine atom; it packs more mass into the molecule than many simple hydrocarbons. These moments, adding the chemical step by step during an experiment and noticing that extra weight, stick with you in a lab memory bank.
The boiling point of 1-Bromohexane hovers around 155°C. That’s pretty high for a six-carbon chain, and once again, the bromine plays a starring role. You can’t just leave this compound in open air near any heat source. This higher boiling range helps if you need a nonpolar solvent with a stronger bond set, or if you’re using it as an intermediate under reflux. At the same time, you have to watch the temperature closely, since inhaling vapors in a small lab with weak ventilation puts your health on the line—headaches, dizziness, and irritation can set in.
On the other side, the melting point dips just below freezing, around −70°C. I’ve never seen it solid in usual room settings—it’s simply not practical unless you cool it with a specialized freezer or dry ice. That means spills stay liquid and should be cleaned up quickly, especially since it turns slick and can make floors dangerous.
If you’ve ever tried to mix 1-Bromohexane with water, you’ve noticed the two layers forming almost instantly. It doesn’t dissolve in water. In college, I saw class experiments with halides separate out like oil and vinegar. The molecule’s long nonpolar tail overrides any slight polarity from the bromine. This makes it easy to isolate from water but harder to clean if something leaks. That’s a double-edged sword: easy phase separation for synthesis, harder cleanup for spills and waste disposal.
On the other hand, 1-Bromohexane mixes well in organic solvents like diethyl ether or chloroform. Anyone who’s spent afternoons in organic chemistry knows these solvents well—the familiar smells and the way they carve up classroom groups into “ether fans” and “chloroform avoiders.” The chemical’s solubility means you can track reactions or purify products using simple techniques like liquid-liquid extraction, a favorite trick of resourceful chemists everywhere.
With all the properties of 1-Bromohexane, no one wants to risk skin or eye contact. Gloves and goggles aren’t optional once you open the container. The liquid’s heavier vapor makes it harder to predict where fumes settle, so keeping a working fume hood or extra ventilation helps. I’ve seen coworkers rush to the eyewash station after splashing organobromines—a harsh reminder to keep safety gear within arm’s reach.
The takeaway: knowing the physical feel and properties of a substance like 1-Bromohexane brings respect for both its usefulness and its hazards. Being aware of just how it behaves in the real world pays off in safe, effective lab work every time you open the bottle.
| Names | |
| Preferred IUPAC name | 1-Bromohexane |
| Other names |
1-Bromohexane n-Hexyl bromide |
| Pronunciation | /ˌwʌnˌbroʊmoʊˈhɛkseɪn/ |
| Identifiers | |
| CAS Number | 111-25-1 |
| Beilstein Reference | 1718730 |
| ChEBI | CHEBI:81323 |
| ChEMBL | CHEMBL16901 |
| ChemSpider | 55309 |
| DrugBank | DB02184 |
| ECHA InfoCard | 03bba471-086e-49a7-9877-3d87b7e0b758 |
| EC Number | 209-598-3 |
| Gmelin Reference | 10745 |
| KEGG | C08295 |
| MeSH | D001950 |
| PubChem CID | 8056 |
| RTECS number | MI8575000 |
| UNII | B7F53B6V2P |
| UN number | UN2342 |
| Properties | |
| Chemical formula | C6H13Br |
| Molar mass | 193.13 g/mol |
| Appearance | Colorless liquid |
| Odor | sweet odor |
| Density | 1.029 g/mL at 25 °C |
| Solubility in water | Insoluble |
| log P | 3.3 |
| Vapor pressure | 0.269 mmHg (25°C) |
| Acidity (pKa) | pKa ≈ 50 |
| Magnetic susceptibility (χ) | -75.0×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.439 |
| Viscosity | 2.084 mPa·s (25 °C) |
| Dipole moment | 1.68 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 356.3 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -66.3 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -4002.7 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02,GHS07 |
| Signal word | Warning |
| Hazard statements | H226, H315, H319, H335 |
| Precautionary statements | P210, P261, P264, P271, P301+P312, P305+P351+P338, P330, P405, P501 |
| NFPA 704 (fire diamond) | 1-2-0 |
| Flash point | 65 °C |
| Autoignition temperature | 180 °C |
| Explosive limits | Explosive limits: "1.1-6.8% |
| Lethal dose or concentration | LD50 (oral, rat): 2900 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 = 2900 mg/kg |
| NIOSH | BJ8925000 |
| PEL (Permissible) | PEL: Not established |
| REL (Recommended) | `REL: NIOSH considers 1-bromohexane to be a potential occupational carcinogen.` |
| Related compounds | |
| Related compounds |
1-Chlorohexane 1-Iodohexane 1-Fluorohexane Hexanol Hexyl bromide |
