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Bromobutane grew out of a surge in organic chemistry during the 19th century, taking its place among straightforward alkyl halides developed through the relentless pursuit of chemists eager to unlock new synthetic pathways. Chemists like August Wilhelm von Hofmann led the way by exploring the patterns and practicalities of simple alkyl halides, giving rise to methods still recognizable in textbooks today. Students fresh to organic laboratories often run into bromobutane during classic substitution experiments. Its preparation and application exemplify how fundamental research yields tools that serve science and industry for generations.
Bromobutane comes in several forms—one-bromobutane, two-bromobutane, isobromobutane—each offering its own quirks. At its core, it remains a four-carbon alkane with a single bromine atom swapped in for a hydrogen. Commercial labs rely on it for its clean reactivity profile and straightforward handling. While not complex by modern standards, its reliability gives it an enduring edge. Researchers keep coming back to bromobutane for its mix of accessibility, safety margin in small labs, and versatile chemistry.
At room temperature, bromobutane exists as a colorless liquid with a faint but sharp, sweet scent. Its boiling point hovers around 101 °C, helping distinguish it from higher members of the bromoalkane family. In the lab, you’ll spot it by its moderate density: heavier than water but not so oily as to cause handling headaches. Chemists respect bromobutane for its mix of solubility—practically insoluble in water but blending well with organic solvents like ethanol and ether. Its reactivity lands in the sweet spot, making it ideal for substitution and elimination reactions without wild side products.
Producers mark each batch of bromobutane with clear specifications, mostly centering on purity (often above 98%), refractive index, and moisture content under 0.1%. These details remain essential for industrial buyers and researchers alike, who rely on consistent starting materials. Safety labeling stays quite direct—chemicals like bromobutane receive hazard identification numbers and pictograms that warn of flammability, health hazards, and environmental impacts. Proper identification on bottles not only meets legal obligations; it also keeps labs running smoothly and safely in the long term.
Making bromobutane doesn’t demand fancy equipment. The classic route starts with butanol, treating it with sodium bromide and sulfuric acid. The sodium bromide and acid together generate hydrogen bromide, which swiftly reacts with the alcohol, swapping the hydroxyl group for a bromine. After this main step, washing, neutralization, and distillation follow. In small academic setups, the process can be scaled up or down as needed, and side products remain minimal with careful temperature control. This approach, unchanged for decades, underlines how reliable chemical methods outlast most technological trends.
Bromobutane steps up in both nucleophilic substitution and elimination reactions. Its C-Br bond breaks cleanly, allowing a wide range of nucleophiles—amines, cyanide, alkoxides—to step in, transforming it into everything from substituted amines to ethers to nitriles. This versatility explains its constant presence in undergraduate synthesis labs and research settings seeking to build new carbon skeletons. Elimination reactions with strong bases kick off olefin formation, while reduction yields butane. Researchers also push surface chemistry and polymer applications by exploiting its alkylating power, not just its basic structure.
Bromobutane answers to several names, including n-bromobutane and 1-bromobutane, reflecting its unbranched structure and bromine’s place on the terminal carbon. You’ll also see the IUPAC name 1-bromobutane, and some suppliers roll out terms like normal bromobutane. These names all point to the same practical material—a versatile four-carbon alkane with a single bromine—and choosing the right synonym mostly helps with sourcing and technical documentation rather than altering any scientific meaning.
Handling bromobutane requires diligence: splash-proof goggles, nitrile gloves, and careful ventilation serve as everyday armor against skin, eye, and respiratory exposure. Its volatility means fumes travel quickly, so working in a fume hood becomes a given. Spills, although infrequent, attract immediate attention due to the potential for skin irritation and central nervous system effects from inhalation. In industry, strict fire protocols must match the flash point hazards, as bromobutane supports combustion. Regulations demand storage away from oxidizers and heat sources, but simple common-sense habits, like double-checking containers and respecting clear labeling, tend to stave off larger incidents.
Industry leans on bromobutane as a cornerstone in organic synthesis. Pharmaceutical companies transform it into anesthetics and antimalarial drugs by way of Grignard reactions and subsequent substitutions. Agrochemical makers start with bromobutane in pesticide intermediates, taking advantage of its straightforward conversion to other functional groups. On the polymer side, it initiates chain-growth processes for specialized resins. University laboratories showcase its flexibility every semester, teaching basic techniques in substitution, extraction, and purification. The common thread across these applications comes down to its ability to reliably link up with a huge range of molecular partners, enabling both new molecules and scalable manufacturing processes.
Efforts in both academia and industry circle around making bromobutane-based syntheses safer and greener. Researchers experiment with less acidic or less wasteful bromination methods, eyeing ways to sidestep the environmental toll of traditional acids and halide salts. Innovations look at photochemical and electrochemical routes, blending old-school reliability with new sensibilities about sustainability. Some labs push into the area of on-demand bromine generation to cut hazardous chemical storage and simplify workflows. This kind of continued curiosity ensures bromobutane remains at the center of discussions about best practices in chemical education and advanced synthesis.
Studies on bromobutane’s impact reveal that acute inhalation hits the central nervous system hardest, prompting dizziness and narcosis at high concentrations. Chronic exposure in animal models ties to liver and kidney effects, but short-term, low-level handling with proper equipment keeps workers and students well-protected. Ongoing research seeks clearer links between environmental release and wider ecosystem effects, especially since bromides can form persistent byproducts. Regulators track permissible limits tightly, and new PPE technology keeps exposure below these thresholds in both classrooms and factories. Direct ingestion presents an emergency, but institutional training around materials like bromobutane keeps such incidents rare.
Bromobutane will likely keep its status as a laboratory staple, propelled by its core reactivity and straightforward production. Emerging green chemistry approaches might offer biocatalytic or waste-reducing alternatives, helping curb environmental burdens tied to large-scale use. In pharmaceutical and materials research, bromobutane takes on added value by enabling modular, step-efficient syntheses of active ingredients and specialized polymers. Digital tracking and data-logistics in supply management could further smooth handling and documentation, reducing bottlenecks and accidental exposures. As science advances, bromobutane stands ready as both a tried-and-true tool and a touchstone for responsible chemistry.
Step into any chemistry lab, and you might spot a clear liquid labeled "bromobutane." Folks outside the field often wonder what place these chemicals have outside those four walls. In labs and factories, though, bromobutane stands out as a real workhorse.
Bromobutane, specifically n-bromobutane, pops up in so many reactions because of its simple structure and reactive bromine atom. I've watched chemists reach for it again and again as a starter ingredient, or "alkylating agent." They use it to tuck the butyl group (that’s four carbons in a row) into other molecules. This trick gets pulled in pharmaceutical labs that design new medicines, in agrochemical development, and when people work on dye and flavor manufacturing.
One use that stands out to me is teaching. University labs often use bromobutane in basic organic chemistry experiments, especially when introducing the concept of nucleophilic substitution, a backbone process for building complex molecules. That hands-on lesson sticks with students because it pulls chemistry out of textbooks and into real life.
Drug companies lean on building blocks like bromobutane for custom chemistry. If I walk through a lab focused on pain medication or cancer treatments, chances are good their shelves carry stable supplies of simple alkyl halides such as this one. They use it to create new links in their chemical structures, sometimes with the goal of improving how the medicine acts in the body or how long it stays effective.
There’s also another side to this story. A chemical like bromobutane can make a huge difference to supply chains. If factories can't rely on steady access to these ingredients, prices and timelines for drugs and specialty products take a hit. Not everyone sees this side of chemistry, but it shapes everything from patient care to food production.
Chemicals that react as quickly as bromobutane don’t come without risks. Skin contact hurts, and breathing it in can irritate the lungs. Years in labs and stories from colleagues show that even good scientists get caught by surprise. Education and good safety gear beat disasters, but not every facility is equally equipped, especially in lower-income areas. There’s a clear message here—safety deserves just as much attention as pure chemistry.
Sourcing safer alternatives sometimes makes sense, but not every chemical has a ready substitute. Some companies recycle leftover chemicals so less gets wasted, and better air filters cut risks for workers. Big changes come with advances in green chemistry. I've spoken with researchers who design new types of reactions that use less toxic materials or produce fewer dangerous byproducts. They often share that cutting waste and exposure is good for both health and business.
Bromobutane usually stays behind the scenes, but its role runs deep in both science education and real-world manufacturing. Keeping supplies stable, training workers, and pushing for cleaner alternatives will make sure that the next generation can use its building power safely and wisely.
Bromobutane is a clear liquid that looks deceptively innocent on the lab bench. It shows up in organic synthesis and undergraduate chemistry labs. Sitting on a shelf, it feels ordinary, but that bottle holds some heavy hazards. If you've spent time in the chemistry lab, you already catch that familiar, sharp smell. That tells me it's volatile—quick to turn into vapor. This is where trouble can start.
One short whiff is enough to remind anyone of bromobutane’s punch. Inhaling its vapors stings the nose and throat and can make your head spin. Breathing too much might even knock you out. The liquid can burn the skin and eyes, leaving behind swelling and redness. I’ve seen students wipe a spill with bare hands and spend the rest of the day nursing painful redness. Long-term exposure brings different worries, from liver stress to possible nervous system effects.
There’s a simple rule from my college lab instructor: If you wouldn’t splash it in your eye on purpose, put your goggles on. Bromobutane makes a convincing case for following this advice. Splash-proof goggles matter more than you’d think, especially when even a drop can cause pain or damage. Gloves are just as non-negotiable. Forgetting gloves means risking weeks of irritated skin. I favor nitrile, since latex doesn’t always stand up to solvents like this one.
Bromobutane slips through air easily, so a well-functioning fume hood saves you from those harsh fumes. Cracking a window doesn’t cut it. If the ventilation fan isn’t humming, I won't start any work. At home, there’s no substitute for lab ventilation, and that’s why I keep work like this far from the kitchen table. Lab coats, buttoned and fitted, keep splashes off street clothes. I learned early to tie back long hair—nobody enjoys the surprise of solvent-soaked hair at the end of a long day.
Planning out each step before touching the bottle keeps surprises at bay. Pour from small bottles, not the big jug. Working with the minimum amount means less vapor, less risk, and less waste at the end of the day. A spill kit close by gives you control. An absorbent pad, gloves, and waste container—a kit I like to prepare before even weighing out chemicals—can make accident cleanup quick.
Every workplace keeps an updated Safety Data Sheet for bromobutane. Reading it matters, because the emergency steps don’t always match what seems obvious. In my lab, we walk through these procedures each semester—where the eyewash station sits, how the shower works, how to call for help. Regular drills sound boring until you’re actually facing a spill or a fire.
Disposing of bromobutane means following strict rules. I bring all used solvents to the chemical waste container, never down the drain or into the trash. Environmental safety isn’t just a paperwork problem—the impact lasts longer than the experiment itself. If you have questions, your lab manager or local environmental authorities can guide you.
Staying safe with bromobutane boils down to respect—for the chemical and the people nearby. It’s about turning caution into habit, not just policy. That's what lets you focus on the science, not the risks.
Picture the clear line between water mixing with sugar and oil refusing to do so. The reason lies in their structures and how the molecules interact. Take bromobutane—a colorless liquid made of four carbons and a bromine atom. Its structure brings up questions. Can it really disappear into water, or does it just float on top?
In chemistry class, we heard the saying: “Like dissolves like.” Water is a polar molecule. Its molecules love to line up into little teams, forming hydrogen bonds with each other or with anything equally loving. Bromobutane, on the other hand, has a big, lopsided molecule. Part of it is non-polar—a carbon-hydrogen backbone that doesn’t like to mingle with water. It only carries a bromine atom at one end, which isn’t enough to change the crowd of carbon and hydrogen. So, bromobutane turns out mostly non-polar.
So, try to mix bromobutane and water in a beaker. You’ll notice two distinct layers—one clear, the other floating on top or sinking, depending on density. Bromobutane’s density sits just above water, so it sinks beneath. Instead of dissolving, it forms a neat layer beneath water, showing how little they like to mix. The numbers back this up. Its solubility sits at about 0.61 grams per liter—barely perceptible. That’s not much compared with ethanol, a similar-sized molecule but one that easily dissolves in water thanks to its polar -OH group.
Some might shrug at the detail about an obscure chemical, but this question pops up in real life. Picture a spill in a lab or factory—will bromobutane spread out in the water supply, or will it form a layer that’s easier to pick up? Also, look at pollution risks. Non-polar chemicals linger in places where polar compounds don’t. If bromobutane leaks into groundwater, it doesn’t mix and move as swiftly as something like alcohol. Cleanup crews have to deal with pockets of chemical, not a diluted solution. Water treatment plants rely on this property. They can separate off these chemicals for special handling.
Having handled chemicals in industrial places, I’ve seen that understanding solubility isn’t just academic. Safe storage asks for double-walled containers and spill trays. Quick access to absorbent sand keeps chemical from spreading. Labeling drums with information about immiscibility with water helps prevent improper disposal.
Getting better at teaching chemical properties early on makes a difference. Kids and adults remember stories and real-world comparisons. A classroom demo, watching bromobutane and water refuse to mix, drives home why some spills are harder to manage, and why waterways need guarding against non-polar pollutants.
Environmental protection relies on people understanding the chemistry they’re dealing with. Governments ask companies using chemicals like bromobutane to keep tight records and train staff to spot risks. On the consumer level, reading packaging and safety sheets pays off. Experts publish research on handling and remediation, building a base of knowledge anyone can use for safer handling.
The solubility of bromobutane in water stands as more than just an academic tidbit. It's a marker of how science shapes real-world safety, clean water, and smart responses to spills and exposure in homes and factories.
You take a clear look at bromobutane in a lab bottle, and it gives off a faint, sweet scent that signals its presence before even reading the label. Room temperature keeps it in a liquid state. Its appearance betrays nothing—it’s colorless, and if you spill it, you’ll notice it evaporates slower than acetone but faster than heavier oils used for machines. So, it lands somewhere in the middle in terms of volatility.
The liquid feels heavier than water. With a density hovering around 1.26 grams per cubic centimeter, a bottle fills your hand with a bit more heft than the same size of plain water. That density, combined with moderate volatility, means bromobutane likes to settle to the bottom in an accidental spill mixed with water. Spotting this firsthand often in undergraduate labs, cleanup takes precision and good ventilation.
Its boiling point lands just above 100°C for the 1-bromobutane isomer—a notch past water, but still in the range where heating on a simple hot plate works. This low boiling point often becomes a feature for folks using bromobutane in organic synthesis. Reflux setups use that number often, letting chemists collect and recycle vapors without needing specialized gear.
People sense the faintly ether-like smell, strong enough to tingle the nose in close quarters. That scent turns out to be more than a curiosity—it warns you to keep the fume hood’s sash low. A quick whiff in a busy teaching lab makes even students scramble for fresh air.
Skin contact does not always sting at first, but after enough time, it can cause irritation. This is no surprise, considering that bromobutane dissolves lipids much like other small alkyl halides. Long sleeves and gloves are a must, which speaks to an ongoing need to reinforce safe habits, especially with newer students or workers.
Bromobutane doesn’t blend easily with water. Pour some in, and it forms a separate, slick layer that floats on top, only mixing in with persistent shaking. This poor solubility in water makes sense—it’s mostly hydrocarbon, with just a bromine atom added. Solvents like ether or alcohol pick it up much more readily, which translates into real lab choices about what glassware or waste containers to use.
In my experience helping set up undergraduate reactions, bromobutane’s willingness to combine with strong nucleophiles pops up again and again. It slips into substitutions with relative ease, which means keeping it away from strong bases or amines unless you want a reaction to kick off unexpectedly.
It’s not enough to simply know these facts as chemistry trivia. Mishandling bromobutane creates real problems—it evaporates into toxic vapors faster than many realize, and its slick nature can cause slips if spilled on smooth tiles. As regulations ramp up, proper containment, ventilation, and disposal grow even more crucial.
In short, the physical properties of bromobutane shape every step from lab bench procedures to storage guidelines. Recognizing the details—its density, tendency to avoid water, moderate volatility, and irritant nature—adds up to safer work and more reliable chemical outcomes in both research and teaching spaces.
Bromobutane catches most folks off guard. It smells faintly sweet but packs a punch well beyond that whiff. Years spent in university labs, watching glassware bubble away behind the fume hood, taught me to respect chemicals like this. Bromobutane shows up in organic synthesis, sometimes gets a nod in undergraduate projects, and always wants extra attention on storage.
The bottle should live in a tightly sealed container, preferably made from glass with a solid, chemical-resistant cap. Metal doesn’t play well with bromobutane, thanks to its reactivity. Place the container inside a dedicated chemical storage cabinet, away from direct light and heat sources. Even a few degrees above room temperature accelerate decomposition, so keep it cool—most sources land on 15-25°C (59-77°F). Refrigeration isn’t a requirement, but folks running a lot of reactions often make that extra investment, especially if the lab’s in a warm climate.
One memory sticks from a summer job at a chemistry lab. A colleague once left bromobutane near a lab window, sunlight streaming in. That bottle was warm to the touch and had a yellowish tint after just a week. Decomposition had started, which risks both the integrity of your experiment and, more crucially, everyone’s safety. Bromobutane is flammable and volatile. Vapors can tickle the nose at first but start causing headaches or worse with enough exposure. If fumes build up, it points to poor sealing or storage, and in a closed space, the fire risk jumps sharply.
Always slap a clear, accurate label onto the storage container. Details should include the chemical’s name, date received, expiration date, and the hazards. In a busy environment, bottles swap hands and shelves routinely. Scraps of tape and faded ink spell trouble. Using clear, chemically resistant labels, with information typed out boldly, reduces mix-ups and keeps the chain of responsibility intact.
Anyone who’s dropped by a hazardous materials seminar hears this on day one: bromobutane stays away from oxidizers, acids, and bases. Even bleach hiding in the same cabinet sets up an accident waiting to happen. Grouping chemicals by class—halogenated organics here, acids and bases over there—nips cross-contamination in the bud. This isn’t red tape; it saves lives and prevents property damage.
New researchers and students often misunderstand just how quickly fumes can build. On more than one occasion, I’ve seen folks forget gloves or goggles “just for a quick transfer.” It only takes one slip to get skin irritation or an inhalation scare. Simple latex or nitrile gloves, splash-resistant goggles, and a working fume hood answer these hazards. Even storage runs smoother with these habits in place every time the cap opens.
If a leak appears or the container feels sticky or smells off, swap it out immediately. Place the compromised chemical inside a larger secondary containment tray, then follow the lab’s chemical waste disposal procedures to the letter. Evacuate if fumes are strong, and never try to mask the odor or just “air it out.” Professional spill cleanup protocols exist for this kind of situation, and calling in backup sends a clear message about valuing team safety and health.
The little things add up, whether that’s making sure each container sits upright or double-checking the cap before leaving for the day. Trusted labs don’t just follow regulations for the sake of the checklist. Their teams care for each other by keeping a close watch on storage conditions and working habits. The most advanced research and sharpest minds rely on solid safety routines—and that includes every bottle of bromobutane on the shelf.
| Names | |
| Preferred IUPAC name | 1-bromobutane |
| Other names |
1-Bromobutane n-Butyl bromide Butyl bromide |
| Pronunciation | /ˌbrəʊməʊˈbjuːteɪn/ |
| Identifiers | |
| CAS Number | 109-65-9 |
| Beilstein Reference | 1209244 |
| ChEBI | CHEBI:28885 |
| ChEMBL | CHEMBL15800 |
| ChemSpider | 6824 |
| DrugBank | DB02185 |
| ECHA InfoCard | 03a6ec93-aa93-4531-96ec-e1a43707b319 |
| EC Number | 208-761-1 |
| Gmelin Reference | 693 |
| KEGG | C01579 |
| MeSH | D001943 |
| PubChem CID | 7868 |
| RTECS number | EO9625000 |
| UNII | U07M3895CO |
| UN number | UN1126 |
| Properties | |
| Chemical formula | C4H9Br |
| Molar mass | 137.02 g/mol |
| Appearance | Colorless liquid |
| Odor | disagreeable |
| Density | 1.276 g/mL |
| Solubility in water | 6.81 g/L |
| log P | 2.9 |
| Vapor pressure | 3.5 kPa (at 20°C) |
| Acidity (pKa) | pKa ≈ 50 |
| Basicity (pKb) | 15.0 |
| Magnetic susceptibility (χ) | -63.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.434 |
| Viscosity | 0.481 mPa·s (25 °C) |
| Dipole moment | 1.66 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 120.3 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | –116.7 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -2877 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02, GHS07 |
| Signal word | Warning |
| Hazard statements | H225, H302, H315, H319, H335 |
| Precautionary statements | P210, P233, P240, P241, P242, P243, P261, P264, P271, P280, P301+P312, P303+P361+P353, P304+P340, P305+P351+P338, P312, P332+P313, P337+P313, P370+P378, P403+P235, P501 |
| Flash point | -6°C |
| Autoignition temperature | 373 °C |
| Explosive limits | 1-9.2% |
| Lethal dose or concentration | LD50 oral rat 3,670 mg/kg |
| LD50 (median dose) | LD50 (median dose): 182 mg/kg (oral, rat) |
| NIOSH | EN8575000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) of Bromobutane is "100 ppm (parts per million)". |
| IDLH (Immediate danger) | 2000 ppm |
| Related compounds | |
| Related compounds |
Butane Chlorobutane Iodobutane Fluorobutane |
