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Long before laboratories featured digital equipment and automation, chemists discovered the reactivity of halogenated alkanes. 1-Chlorobutane, also called n-butyl chloride, entered the catalog of useful chemicals as researchers explored alkyl halides in the late 1800s. Organic chemistry textbooks documented it as a tool for understanding substitution mechanisms and reaction pathways. Early industrial chemists found that large-scale alkylation grew easier with sturdy reagents like 1-Chlorobutane. Now, it stands as a common reference material for both industrial and academic research. Its story follows shifts in manufacturing, growing from lab-bench curiosity to everyday chemical stockroom mainstay.
1-Chlorobutane offers a straightforward carbon backbone with a single chlorine atom at the terminal position. Its CAS number is 109-69-3, and it holds a key spot among primary alkyl chlorides. In the plant, workers handle it as a clear, colorless liquid, recognizable by a distinct, sharp odor. Product grades range from technical to high-purity, depending on downstream uses. Bulk shipments rely on drum or tank truck packaging, and regulatory labeling must flag its flammability and toxicity hazards. Across markets, it’s most often sourced as a foundational intermediate for synthesizing other chemicals—think pharmaceuticals, surfactants, and rubber additives.
1-Chlorobutane’s four-carbon chain carries weight, clocking in at a molecular weight of 92.57 g/mol. It boils at about 78 °C, freezes at -123 °C, and delivers a vapor pressure near 200 mmHg at 20 °C. This compound stays out of water; its immiscibility explains why containment matters during use. Chlorine’s presence boosts its density to around 0.89 g/cm³ at room temperature, above that of unhalogenated butane. Chemical workers note its flammable nature, supporting clean blue flames, and watch for volatility that increases the chance of inhalation exposure. The carbon-chlorine bond, polar and readily attacked by nucleophiles, makes it valuable in substitution and elimination reactions. Generating an alkylating agent with predictable, well-understood behavior helps chemists build more complicated molecules.
Manufacturers spell out composition, purity, and water content for 1-Chlorobutane. For demanding uses, purity above 99% is expected. Testing protocols, including gas chromatography, confirm identity and exclude residual isomeric byproducts like 2-chlorobutane. Chloride ions, acidity, and nonvolatile residue concentrations get tabulated for buyers in pharmaceuticals or electronics. Global shipment rules—based on GHS, OSHA, and Transport of Dangerous Goods regulations—require hazard pictograms and signal words such as “Danger.” Even with rigorous transport standards, chemical handlers still train for potential spills, using vapor-tight goggles and nitrile gloves. Labeling never skips irritation and environmental impact warnings.
Most 1-Chlorobutane comes from straightforward chlorination of n-butanol, often with hydrochloric acid or thionyl chloride. Smaller labs use sodium chloride and sulfuric acid to produce hydrogen chloride gas—then pass that gas through butanol under reflux, collecting rain of chlorinated product. Some sites favor direct chlorination of butane, but this requires precise control to hit the right substitution and avoid over-chlorinating. Older textbooks report phosphorus trichloride as a classic method, now less common for bulk manufacturing due to cost and waste disposal headaches. Today, high-output facilities select processes that minimize hazardous byproduct formation, cutting costs and reducing regulatory fines.
Chemists see 1-Chlorobutane as a launching pad for other molecules. The primary carbon, bonded directly to chlorine, undergoes nucleophilic substitution, making alkylation and etherification reactions efficient. Grignard reagents form when butyl chloride meets magnesium, opening paths to alcohols and carboxylic acids after further functionalization. Sulfide, cyanide, and ammonia reagents swap in their functional groups by displacing chlorine. In elimination reactions, it gives 1-butene or even trans-2-butene in the presence of strong bases. Its flexibility supports synthesis of plasticizers, fuel additives, insecticides, and custom organometallic complexes.
Common synonyms dot the literature: n-Butyl chloride, Butane-1-chloride, 1-chlorobutan. Older catalogs sometimes call it chloromethylethylethane, revealing naming conventions from decades past. Today, “1-Chlorobutane” and “n-Butyl chloride” dominate safety sheets, batch records, and data tables. This compound might pop up under trade names in branded blends for surface chemistry or polymer industries. Skilled operators know these aliases because substitutions or purchasing errors can trigger unwanted isomer formation—clear naming helps prevent mixing up primary and secondary chlorides.
Attention to safety shapes every contact with 1-Chlorobutane. The liquid gives off hazardous, flammable vapors at room temperature, requiring ignition controls and grounded containers. Inhalation brings on cough, dizziness, and in higher doses, narcosis. The molecule’s volatility and poor water solubility mean spills vaporize quickly but still stick around in closed spaces. Chemical hygiene plans enforce tight-fitting goggles, chemical-resistant gloves, and fume hoods for every procedure. Storage never places it near oxidizers or heat sources, and empty drums get cleaned before re-use. Waste disposal follows environmental rules for chlorinated hydrocarbons, passing through specialized facilities to destroy persistent pollutants. Worker training covers not just PPE use, but emergency spill and fire protocols, saving health and reducing costly downtime.
1-Chlorobutane’s versatility supports a wide slate of commercial products. Surfactant manufacturers rely on it for quaternization reactions, bridging butyl moieties onto amines and delivering superior detergency. In rubber production, it serves as a functionalizing chain end, anchoring additives that modify elasticity and durability. Agrochemical developers use it to introduce functional groups onto active ingredients for pesticides and herbicides. Its role as a starting alkylating agent in pharmaceuticals means it appears in antihistamines, anticonvulsants, and cardiovascular drugs. Research labs keep it stocked for organic synthesis schemes, from undergraduate teaching to patent-driven innovation. Even materials scientists use it to surface-modify nanoparticles and design new composites. Having such a direct, reliable alkyl chloride cuts trial-and-error steps out of chemical engineering workflows.
Ongoing research with 1-Chlorobutane focuses on safer reaction conditions, greener conversion routes, and more efficient use as a building block. Scientists now look at alternative chlorination catalysts that cut out hazardous co-products, and they’re tinkering with one-pot, solvent-free syntheses for reduced environmental impact. The molecule grabs attention in physical chemistry—models of its boiling and vapor-pressure data refine predictive software for safety engineers. Academic labs also use it to teach structure-reactivity relationships and separation techniques, from simple refluxes to modern flash chromatography. Research into catalyzed reactions finds 1-Chlorobutane a favorite for demonstrating SN2 versus E2 competition, key to understanding core organic mechanisms. As regulatory standards climb, industry-backed projects explore biodegradable routes and emission-reducing production methods that keep pace with sustainability commitments.
Toxicology studies mark 1-Chlorobutane as both an irritant and a narcotic at moderate exposure. Inhalation trials on rodents reveal central nervous system impacts and minor liver enzyme changes after prolonged contact, boardroom reminders for strict exposure limits. Dermal absorption data reinforces glove use, since repeated skin contact produces dermatitis and inflammation. Water-soluble metabolites excreted by exposed animals show that it breaks down in the body, but neither rapidly nor without some stress to the detox circuits like cytochrome P450. Decision-makers in chemical management scan these findings to set workplace exposure limits—occupational standards across North America and Europe aim for time-weighted averages that avoid chronic health effects. Detailed breakdown products get tracked for environmental toxicity; some chlorinated intermediates persist in water or soil, earning extra scrutiny from regulatory inspectors.
Advances in green chemistry push future work on new production methods for 1-Chlorobutane, targeting safer, less energy-intensive processes to meet climate and workplace safety goals. Research on catalytic, non-solvent synthesis could cut energy costs and hazardous byproduct loads. As demand grows from custom pharmaceuticals and niche materials, smaller, modular manufacturing plants might pull it together on-site as a just-in-time reagent, slashing logistics and minimizing accident risk in transit. Technology from automated process monitoring and AI-powered quality control points toward sharper operational oversight, stopping off-spec batches before they leave the plant. Regulatory shifts will likely require manufacturers to document life cycle emissions, pushing sustainable sourcing and waste handling higher on the priority list. Chemists and plant managers in the next decade face ongoing challenges around safe handling and regulatory compliance, but smart innovation can keep 1-Chlorobutane a useful, manageable tool for the modern chemical landscape.
1-Chlorobutane belongs to the family of organochlorine compounds. It looks like a clear, colorless liquid, carrying a mildly sweet odor that’s easy to spot in any well-ventilated lab. The chemical structure—a four-carbon linear chain with a chlorine atom hooked onto the end—grants it just the right balance of reactivity for both research and industry. After years in a chemistry lab, you start to appreciate which substances pull the most weight in synthesis work, and this one is a regular in practical applications.
Most memorable lab sessions involved reaching for a bottle of 1-chlorobutane, especially during nucleophilic substitution reactions. It dissolves lots of organic compounds, making these reactions possible on a larger scale. Organic chemists value reliable solvents that don’t interfere with delicate reactants. And 1-chlorobutane consistently meets that need, especially in the textbook SN2 and SN1 reactions used to produce everything from pharmaceuticals to everyday plastics.
This compound’s real forte lies in its ability to act as an intermediate. Manufacturers count on 1-chlorobutane for the production of amines, alcohols, and thiols. My experience in industry research showed me how often these building blocks land in the synthesis of herbicides, insecticides, and even flavors. The chlorine atom, bound on the outer end, can be swapped for other functional groups, which creates hundreds of possible molecules from this starting material. That chemical versatility explains why many chemical supply catalogs feature it high on their lists.
After moving from academia into the world of polymer manufacturing, I spotted 1-chlorobutane doing a different job: helping stabilize polymer chains and control the properties of specialty plastics. In rubber manufacturing, chemists incorporate it to improve softening and flexibility. It’s not as flashy as other ingredients, but it ensures the final product stands up to wear and tear from daily use—think car tires, medical tubing, even the coatings inside electrical wires.
Work in fuel research introduced me to another side of 1-chlorobutane. Gasoline researchers have mixed it into fuel blends to check ignition properties or tweak combustion. It can act as a reference compound while testing octane ratings. In a sector where every fraction of a percent matters for engine performance and emissions, even small-volume chemicals can mean the difference between a patent and a recall.
People working with 1-chlorobutane need to treat it with care. Although commonly used in manufacturing, it carries health risks if inhaled or spilled on skin. I’ve seen strict safety sheets governing its use, and workplace training focuses on storing it away from flames or static sparks. Investing in proper ventilation and personal protective gear—like gloves and goggles—goes a long way toward protecting both workers and the environment from unwanted exposure.
One promising direction involves designing greener alternatives or improved recycling systems for organochlorine waste. I’ve heard about pilot projects that recover halogenated solvents for reuse, reducing contamination and disposal concerns. Tightening up regulatory standards, together with industry self-regulation, encourages a culture where efficient chemical use matches responsible stewardship. Tackling these challenges head-on means future generations of chemists can keep making scientific progress without trading away safety or sustainability.
Grabbing a bottle of 1-chlorobutane off the shelf in a lab, most people barely glance at the details beyond the name on the label. I remember my first year working with organic solvents—the long string of safety checks and prep seemed like overkill. Then I saw a reaction overheat and spray half-melted glass onto the fume hood window. Precision isn’t about just following a rulebook; it’s about keeping yourself and your work safe.
The boiling point of 1-chlorobutane clocks in around 78°C (172°F). This isn’t a trivial piece of trivia. Knowing it means the difference between clean distillation and an evacuation due to unexpected fumes. It impacts safety measures, the way ventilation is set up, and how you prep for storage.
Every time you use 1-chlorobutane, you’re handling a chemical with both value and risk. Its boiling point matches up closely with water, but it behaves nothing like it. The low boiling point tells you that it evaporates easily, so even a slight rise in temperature can fill the air with vapors. If you ever worked in a high school chemistry lab, you remember that sharp, almost sweet fragrance of chlorinated solvents. Without knowing where boiling starts, slips happen—maybe a flask explodes, or the air in the lab smells wrong. Health is at stake, and property, too.
Labs with poor airflow or careless temperature control make it easy to miss the warning signs until it’s too late. In my experience, keeping a close eye on boiling points isn’t just for exams or manuals. It’s about making sure that a late night at the bench doesn’t end with a chemical burn, migraine, or call to the fire department.
Take a look at data from chemical supply catalogs like Sigma-Aldrich or PubChem. The listed boiling point for 1-chlorobutane is reliably about 78°C. That means any heating above this, without knowing what’s at stake, leads straight into a danger zone for both the handler and the environment. Exposure to the vapor can cause eye, nose, and throat irritation. If you work in a crowded lab, it doesn’t take much for one person’s mistake to turn into everyone’s emergency.
Production industries that rely on 1-chlorobutane use this boiling point to design their equipment. Tank venting, distillation columns, vapor recovery—these pieces only work right if people respect the boiling point. Overlooking it costs time and money in wasted product, equipment repairs, or full shutdowns after accidents.
Clear safety protocols help. Good ventilation, regular equipment checks, personal protective gear, and never pushing the temperature just to save time—these are habits that prevent disaster. Back at my university, one old professor drilled it in: Don’t let the boiling point surprise you. Double-check temperatures, keep an eye on insulating barriers, and always store solvents cool, dark, and dry. In my own practice, I log every solvent’s properties before beginning a new synthesis or purification—critical steps spelled out by green chemistry standards.
Technology lends a hand, too. Automated temperature cut-offs, fume hoods with real-time vapor sensors, and digital process logs blunt human error. Even small investments in good thermometers or online property databases pay off when one misstep could trigger a fire alarm or a hazardous exposure.
Ultimately, it’s about respect for the chemistry. The data’s already out there: the boiling point of 1-chlorobutane is well-known and easy to access. Turning that information into safe, productive work is a responsibility shared by everyone who handles it, from students to plant managers.
1-Chlorobutane might sound like science class material, but it’s a chemical used in real-world manufacturing. Factories rely on chemicals like this one to make plasticizers, pharmaceuticals, and sometimes as a solvent in labs. The issue comes up when people start working with or near it without solid information on what it can do to the human body.
No one likes to breathe in stuff with “chloro” in the name, and for good reason. The vapor from 1-Chlorobutane can irritate eyes, nose, and throat. If you ever visit a plant that deals with these types of chemicals, folks often mention a strong, sharp smell in the air. Government studies back this up, showing even short-term exposure can cause dizziness and headaches. Higher levels may lead to more serious issues like confusion or even loss of coordination. It makes sense—firms like the CDC and EPA don’t toss out health warnings for nothing. Anyone who spills this stuff on their skin also risks redness and a burning sensation. It’s far from the kind of job hazard you want to ignore.
Some chemicals wash off easily or break down quickly. 1-Chlorobutane doesn’t play by those rules. The body absorbs it through the lungs and skin, then breaks it down in the liver. This process can create byproducts that are not well understood, leaving scientists with more questions than answers. What does show up in published studies? Workers who get exposed often, especially without good protection, may report persistent coughing, nausea, and lightheadedness. It’s not a stretch to see why health agencies urge caution, especially since there isn’t much long-term data on cancer risk but there’s enough concern to take it seriously.
It’s easy for management to post a safety sign and hand out thin gloves, but that won’t cut it. People need training on real risks, and access to solid protective gear. Good ventilation matters too—I’ve seen too many places rely on a window fan and hope for the best. Let’s not forget accidental splashes or spills, which are almost guaranteed in a busy work environment. That’s why it’s smart to have clear emergency steps and eye wash stations placed where they are actually reachable, not stuffed in a locked supply closet.
Cutting down on risk means more than following the legal bare minimum. Companies should give regular health screenings to workers who handle chemicals like 1-Chlorobutane. Employees also need straightforward information, not just thick binders of material safety data sheets that few people have time to read. Swapping out 1-Chlorobutane for less risky compounds can make a big difference, where possible. Simple steps like these protect not only workers, but also their families—fewer cases of chemicals coming home on clothing, fewer health scares down the road.
We all rely on products made with chemicals, but that doesn’t make exposure a background concern. Health hazards from 1-Chlorobutane show up in emergency room visits, workers struggling with nausea on the job, and companies facing legal trouble. Real people face real risks every day. With basic respect and smart policies, those dangers drop way down. Respecting workers’ health never gets old.
Anybody working with chemicals long enough learns to take every label seriously. With 1-chlorobutane, there’s a sharp, sweet smell that hints at what’s inside the bottle. This isn’t just another workplace solvent; it’s flammable, volatile, and not too gentle on your skin or lungs. I remember the first time I cracked open a small container, and the fumes caught me by surprise. That taught me respect, not just for the liquid but for every step between storage and disposal.
Let’s start with the basics: 1-chlorobutane needs a cool, dry, and well-ventilated spot. Storage around 15 to 25°C helps avoid any hiccups with pressure build-up or leaks. Fans in the area keep fumes from turning the air into a health hazard. Direct sunlight raises both the temperature and the odds of a chemical reaction, so a shaded or indoor storage room far from heat sources beats any open shelf.
A good chemical cabinet, made of metal or polyethylene, holds up well. It should close tightly and have a clear label. At my old lab, we always made sure labels faced outward and warnings didn’t wear off—small habits, big payoff. If a bottle leaks, it can corrode shelving or mix with air, so make sure the cap is tight and containers have no cracks or stains.
1-chlorobutane catches fire easily. Static electricity, open flames, or even lazy wiring turn a routine day into a disaster. I’ve seen colleagues carry out regular inspections, and I do the same: electrical sockets get covered, no smoking signs go up, and nothing sparking stands nearby. Fire extinguishers made for chemical fires, like those with dry powder, should stay within arm’s reach—water only spreads the solvent.
Acids, strong oxidizers, and alkalis don’t play well with 1-chlorobutane. Mixing with the wrong chemical creates toxic fumes, corrosive byproducts, or worse, an explosion. Good practice means storing it on its own shelf, apart from anything reactive. Color-coded storage bins help, and regular checks catch any cross-contamination early.
Gloves, goggles, and lab coats seem obvious, but I’ve seen enough shortcuts taken after a long day. A spill on bare skin burns quick—ask anyone working with organics. Real safety comes from training. A lab manager or safety officer makes a difference, especially if they know the quirks of each solvent on the shelf.
Spill kits, eyewash stations, and proper ventilation save lives. Every worksite should have chemical spill kits clearly visible. Accidents don’t come with warnings, so having an emergency contact list and clear exit routes written down and posted helps everyone keep their heads straight in a panic. Whenever a new shipment arrives, updating the inventory and Safety Data Sheets avoids mix-ups.
The story of 1-chlorobutane storage isn’t new, but it’s easy to ignore the simple steps that keep people safe. Day-to-day attention to conditions, keeping chemicals apart, wearing the right gear, and always preparing for accidents don’t just meet the rules—they protect health, jobs, and peace of mind.
Most people don’t run into 1-chlorobutane on a daily basis unless they’re in a chemistry lab or in the middle of a manufacturing plant. Reach for a bottle of the stuff, and it greets you with a clear, almost watery look. Pouring it out, the liquid flows with a slight slickness, much like many solvents I’ve used in college practicals. It’s got a distinct, biting odor that says “handle with care.”
The boiling point for 1-chlorobutane sits around 78°C. On a hot summer day, that number means this chemical won’t stay put for long if left open. It evaporates easily. Pop a thermometer in and you’ll see the temperature climbs quickly when you apply heat—something lab folks have to keep an eye on. The density hovers a bit above water at 0.88 g/cm³, so it floats on some solvents but sinks in others. It won’t dissolve in water, which says a lot about its relationship with nature. Try to mix it, and it just separates out, forming a slick layer on top.
The colorless look, the higher-than-water density, and the snappy smell all come together to tell anyone who’s paying attention: this isn’t as harmless as water or alcohol. Its physical properties set the stage for safety measures in labs and factories. Engaging with it without gloves ends poorly, as the strong solvent properties can irritate skin. The rapid vaporization poses inhalation risks too. These are just a few reasons why storerooms keep it in tightly sealed containers, far from flames or children.
Chemically, 1-chlorobutane wears the badge of an alkyl halide. It has a four-carbon backbone wearing a single chlorine atom on its end—simple, but highly reactive in the world of organic chemistry. That reactive chlorine gives it a personality: under the right circumstances, it replaces itself with other atoms. Reactions like nucleophilic substitution chew through 1-chlorobutane as if it’s designed to be changed. Toss in a strong base and it will undergo elimination, kicking out the chlorine and forming a double bond.
Using 1-chlorobutane in syntheses always demanded patience from my classmates. It tends to react with sodium metal to form sodium chloride and butane, which led to a few fireworks in my undergraduate days—nobody appreciates how violent that reaction gets without seeing it first-hand. This reactivity makes it valuable for building more complicated molecules in the lab or in bigger-scale drug manufacturing. Without this molecule, several industrial syntheses would stall or cost a lot more to accomplish.
Storage becomes a real talking point. The chemical catches fire easily, so manufacturers highlight its flammability for good reason. Improper storage has caused incidents: every chemist hears stories about containers swelling in the summer heat. On the environmental side, spills spread fast and stick around since they don’t dissolve well in water.
To lessen risks, facilities install proper ventilation, seal containers, and use chemical-resistant gloves. Years in the lab taught me that even a moment’s carelessness around halogenated solvents leads to long clean-up sessions or worse, a visit to the clinic. In the right hands, though, 1-chlorobutane finds its place in the synthesis of pharmaceuticals, fragrances, and specialty chemicals. With careful handling and a respect for both its physical and chemical features, it stands out as a workhorse molecule.
| Names | |
| Preferred IUPAC name | 1-Chlorobutane |
| Other names |
n-Butyl chloride Butyl chloride 1-Chlorobutan Butane, 1-chloro- n-Butane chloride |
| Pronunciation | /ˈklɔːr.oʊ.bjuː.teɪn/ |
| Identifiers | |
| CAS Number | 109-69-3 |
| Beilstein Reference | 1720236 |
| ChEBI | CHEBI:35721 |
| ChEMBL | CHEMBL16867 |
| ChemSpider | 6829 |
| DrugBank | DB14006 |
| ECHA InfoCard | 100.003.965 |
| EC Number | 203-691-9 |
| Gmelin Reference | 8017 |
| KEGG | C01848 |
| MeSH | D001821 |
| PubChem CID | 8037 |
| RTECS number | EJ8575000 |
| UNII | 9G1I0A8H3T |
| UN number | UN1127 |
| Properties | |
| Chemical formula | C4H9Cl |
| Molar mass | 92.57 g/mol |
| Appearance | Colorless liquid |
| Odor | Aromatic |
| Density | 0.886 g/mL at 25 °C |
| Solubility in water | Slightly soluble |
| log P | 1.81 |
| Vapor pressure | 10.7 kPa (at 20 °C) |
| Acidity (pKa) | 15.0 |
| Basicity (pKb) | > 15.3 |
| Magnetic susceptibility (χ) | -62.0·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.403 |
| Viscosity | 0.685 mPa·s (at 20 °C) |
| Dipole moment | 1.72 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 229.6 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -146.5 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -2765.0 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02, GHS07 |
| Signal word | Warning |
| Hazard statements | H225, H315, H319, H335 |
| Precautionary statements | P210, P261, P271, P301+P312, P304+P340, P312, P403+P233, P501 |
| NFPA 704 (fire diamond) | 1-2-0 |
| Flash point | -6 °C |
| Autoignition temperature | 245 °C |
| Explosive limits | 1.8–10.1% (in air) |
| Lethal dose or concentration | LD50 oral rat 3,600 mg/kg |
| LD50 (median dose) | LD50 (median dose): 2730 mg/kg (rat, oral) |
| NIOSH | EO8400000 |
| PEL (Permissible) | 100 ppm (300 mg/m3) |
| REL (Recommended) | 100 mg/m³ |
| IDLH (Immediate danger) | 800 ppm |
| Related compounds | |
| Related compounds |
Butanol Butyl chloride Butyl bromide Butyl iodide 1-Bromobutane 1-Iodobutane |
