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Acyclic alcohols have woven into the story of industrial and organic chemistry since the days before their structures had names. Ethanol, the most familiar of the group, traces its roots to fermented beverages in ancient civilizations. Later on, distillation brought higher purity and new uses, from medicine to fuels and solvents. The recognition of alcohols as a distinct class grew alongside organic chemistry in the 19th century, led by breakthroughs from Justus von Liebig and Hermann Kolbe. Their careful studies opened the world to countless compounds sharing the recognizable -OH group. Chemists then pushed beyond alcohols from natural sources, synthesizing new acyclic alcohols for industrial processes, plastics, and fuels. Some of these, like methanol and butanol, entered the modern world not just as curiosities, but as economic engines driving industries from adhesives to biofuels. Alcohols, acyclic or otherwise, represent more than a compound—each marks a chapter of science, trade, public health, and global industry.
Acyclic alcohols are simply alcohols with open-chain carbon structures, distinguished from their cyclic cousins. They range from the one-carbon methanol up through longer chains like pentanol and octanol. Methanol became central in the shift from wood distillation to large-scale synthesis using carbon monoxide and hydrogen. Ethanol continues to dominate pharma, beverage, fuel, and cleaning sectors. Butanol, isopropanol, and hexanol each bring unique traits to surface coatings, cleaners, nylon intermediates, and lubricants. Over a hundred named acyclic alcohols fill chemical catalogs today. Their popularity flows from how the hydroxyl group interacts with other chemicals, dissolves a host of substances, and alters boiling and melting points in ways no hydrocarbon can match. In practice, each acyclic alcohol finds its home in blend ratios and manufacturing tolerances that shape entire industries.
You know an acyclic alcohol when clear, colorless liquids fill the flask with a distinct alcohol smell—some sweet, some sharp. Their boiling points start low with methanol, climbing up the chain with each added carbon. Volatility drops and viscosity rises along the series. Most mix well with water up to four carbons, but solubility tails off with longer chains—octanol barely mingles. That’s a big reason why ethanol cleans glass while octanol supports cosmetics and perfumes. Chemically, acyclic alcohols play nice with both acids and bases. Their -OH group participates in hydrogen bonding, leading to higher boiling points than alkanes. Acyclic alcohols also act as versatile starting points for oxidation, ether formation, and esterification. Flammability, especially for the lower alcohols, deserves respect in any lab or factory handling.
Every bottle of acyclic alcohol should tell you more than just its common name. Purity, water content, and the presence of trace contaminants like aldehydes or ketones all matter. For pharmaceuticals and food production, only the highest grades work. Technical grade suits industrial needs, but even small impurities can ruin a polymer batch or batch of flavoring. Labels usually give chemical formula, physical constants like boiling point, flash point, and density. Safety icons, UN transport codes, and storage recommendations help handlers prevent accidents. With growing scrutiny from regulators, even the origin—bio-based, synthetic, or recycled—may appear on labels as markets evolve to reward lower-carbon options.
Methanol once came from destructive distillation of wood, but now production giant plants convert synthesis gas—carbon monoxide and hydrogen—into methanol under pressure with a metal catalyst. Ethanol, for all its familiarity as a drink, owes its industrial volumes to fermentation of sugars using yeast, or synthetic hydration of ethylene. Modern processes favor continuous operation, high efficiency, and catalysts recycled within the loop. Butanol family alcohols frequently use hydroformylation followed by hydrogenation, or microbial fermentation in biofuel plants. Small-batch labs still prepare rare or uniquely branched alcohols with classic organic reactions—Grignard additions to carbonyls or catalytic reduction—passing the torch from theory to scalable practice.
Acyclic alcohols function as flexible platforms for further chemistry. Oxidation turns alcohols into aldehydes and carboxylic acids—acetic acid from ethanol being the classic demonstration. Dehydration provides routes to alkenes, important in the plastic industry, while substitution swaps the OH group for a halogen and sets up more interesting molecules. Fischer esterification brings alcohols together with acids to form esters, those familiar in fragrances and solvents. Ethers emerge from acid-catalyzed coupling of two alcohols. Chemical companies depend on these predictable reactions to form polymers, antifreezes, detergents, and flavors. Robustness and versatility help alcohols remain the nucleus of synthetic pathways.
Each acyclic alcohol goes by a few common aliases reflective of its context. Methanol also answers to wood alcohol or carbinol, while ethanol might turn up as ethyl alcohol, grain alcohol, or spirits—names shifting between lab and liquor store windows. Isopropanol holds court as rubbing alcohol, 2-propanol, or sec-propyl alcohol depending on region and use. Butanol branches into n-butanol, iso-butanol, both valuable but slightly different in effect and industrial niche. Synonyms serve more than convenience; they remind us chemistry touches every corner, from pharmacy to fuel pump to cleaning closet, under a dozen names.
Handling acyclic alcohols without respect results in disaster—flammable vapors ignite from static sparks, and toxic effects come long before a spill starts to smell. Methanol, for instance, once slipped into counterfeit spirits, blinds or kills with tiny doses. Ethanol intoxicates, but even industrial fumes deserve caution. Regulatory standards spell out ventilation needs, fire precautions, maximum exposure limits, and protective gear for workers. Process plants set up sensors, spark-free tools, and spill containment features by the book, all under environmental and health agencies that don’t hesitate to fine violations. Buyers, from paint formulator to cocktail bar, depend on upstream compliance so downstream uses remain safe. Tech innovation now tracks leaks and emissions with sensor networks, limiting risks even under heavy use.
No shelf sits untouched by acyclic alcohols. Methanol runs as a solvent, a feedstock for formaldehyde, and even steps up in racecar fuels. Ethanol’s versatility lands it in sanitizers, disinfectants, beverages, cosmetics, and alternative fuel pumps. Isopropanol remains the universal cleaning fluid for glass, electronics, and pharmaceuticals. Butanols end up in paint solvents, plasticizers, and hydraulic fluids. Longer chain alcohols like octanol and dodecanol stay out of drinks, but persist in surfactants, lubricants, and high-performance materials. Consumer familiarity revolves around surface cleaning and hygiene, but behind the curtain, acyclic alcohols push innovations in drug synthesis, renewable fuels, and fine chemistry every day. When prices shift or shortages hit, ripples spread across manufacturing, medicine, and even global supply chains.
Today’s labs rarely rest on the achievements of pure alcohols; new methods seek efficiency, sustainability, and applications nobody imagined fifty years ago. Research now explores engineered microbes to ferment waste gases into longer-chain alcohols, building on the rising tide of biomanufacturing. Green chemistry forces efficiencies in catalytic hydration and oxidation to slash waste and energy demand. Some teams hunt for novel alcohol-based solvents that extract active ingredients while reducing environmental toxins. Advances in separations, such as membrane-based distillation, chase better energy profiles for large-scale purification. Electronics and energy storage industries pour resources into alcohol-derived additives that boost battery life or corrosion resistance. Regulatory trends push researchers to develop alcohols from renewable sources and with lower toxicity profiles, aiming to displace petrochemical products without sacrificing performance.
Toxicologists monitored acyclic alcohols for generations, learning through tragedy and careful studies. Methanol stands as the poster child for stealthy danger; ingestion or inhalation causes blindness, organ failure, and death at doses smaller than many industrial chemicals. Ethanol’s effects on the human body spawned entire research fields and legal frameworks, as both its recreational use and abuse soak into culture worldwide. Isopropanol shares anesthetic and toxic profiles—effective as an antiseptic, sickening in cocktails. Long chain alcohols fade in acute toxicity but can disrupt aquatic environments if poured down drains or spilled from tankers. Animal studies, population surveys, and occupational health audits build the facts that shape regulations and workplace controls. Every leap in production volume brings new scrutiny, asking whether substitutes or safeguards could cut risk for workers and communities.
The world’s climate push, renewed focus on sustainability, and new markets all circle back to acyclic alcohols. Bioethanol and biobutanol grab headlines as gasoline extenders, promising to cut tailpipe emissions without sacrificing infrastructure. Green chemistry methods for alcohol synthesis continue to drive down carbon footprints, even as demand rises in developing industries. Synthetic biology could deliver specialty alcohols from waste or CO2, taming both emissions and supply chains. Researchers race to build molecules with unique properties—low volatility, non-toxicity, tunable solubility—for electronics, medical imaging, and custom materials. Demand won’t fall: as healthcare needs stricter sanitization, transport pivots to green fuels, and supply chains decouple from geopolitics, acyclic alcohols stand ready for reinvention. The challenge rests with policymakers, engineers, and innovators, who must balance the benefits with honest risk assessment and transparent stewardship.
Some of the best lessons I ever learned about chemistry started in a high school lab. I remember pouring out clear liquids, watching reactions, and then realizing many chemicals had strange names but simple uses in daily life. One of those lessons started with the word “alcohol.” People might immediately think of bottles behind a bar, but the story in chemistry goes further. Alcohols show up in many products around the house, in medicine cabinets, and even in cars as fuel additives. Among all those types, acyclic alcohols hold a solid place in science and daily routines.
Acyclic alcohols follow a straight or branched chain skeleton, built mostly from carbon and hydrogen, ending with at least one –OH group. Unlike ring-shaped (cyclic) alcohols, acyclic alcohols have open chains. The most recognizable example is ethanol, the alcohol in drinks, hand sanitizers, and even fuel blends. Then there’s methanol, often found in antifreeze and as a solvent. Both sit front and center in classrooms and industries due to their roles in synthesis and daily applications.
Look around any medical facility and you see hand sanitizers, disinfectants, and cleaning sprays. Ethanol and its cousins get the job done: evaporate quickly, kill germs, and leave less residue. In the home, rubbing alcohol serves as a first aid staple. Outside these spaces, acyclic alcohols help engines run cleaner. Ethanol blends with gasoline lower emissions—offering a small step toward greener energy use. Reports from Renewable Fuels Association show nearly all gasoline in the U.S. contains up to 10% ethanol. This reduces reliance on fossil fuels and supports cleaner air.
Growing up, I watched a neighbor accidentally ingest methanol from mislabeled spirits—a hard lesson about the difference between drinkable and industrial alcohol. Methanol, while useful for antifreeze and solvents, turns toxic in even small amounts. It can cause blindness and organ failure. Education about these differences matters. Labels and regulations save lives and ensure proper use.
Industries count on acyclic alcohols in daily operations. Paints, cosmetics, fuel, and pharmaceuticals often start or end with these molecules. Some beauty products rely on ethanol as a carrier or solvent. Factories lean on isopropanol for cleaning machinery due to its rapid evaporation and effectiveness in grease removal. Even in labs, researchers use acyclic alcohols to purify and analyze compounds. The sheer range keeps demand steady, and companies constantly search for better ways to produce alcohols with fewer emissions and less waste.
Large-scale production creates its own environmental puzzle. Traditional methods rely heavily on fossil fuels, heating, and pressurized systems. Companies are researching new catalysts and fermentation techniques to make production cleaner. Recently, biorefineries began converting agricultural waste and sugars into ethanol, which cuts carbon footprint and gives farmers an extra source of income. This technology doesn’t just make for cleaner fuel; it stirs up local job markets and keeps waste out of landfills.
Education stands out as another solution. Understanding which alcohols to use—and how—is as important as producing them safely. Outreach from health authorities and clearer packaging protects the public and saves emergency rooms from exposure cases. Investing in better labeling, staff training, and public information helps keep people out of harm’s way without slowing progress in science and industry.
From antiseptics to alternative fuels, acyclic alcohols remind us every day that chemistry isn’t just for textbooks. It shapes habits, safety, and innovation, one molecule at a time.
Whether out in the world or at home, acyclic alcohols show up everywhere. These are the straightforward types of alcohol, with their carbon atoms linked up in open chains—think ethanol and methanol as prime examples. You’ll find their fingerprints across a wide spread of industries, supporting tasks people tend to take for granted. Their chemical backbone makes them reliable, but real-world value comes from what folks do with them.
Ethanol today powers not just late-night cleaning marathons but thousands of cars and trucks. Folks blend ethanol with gasoline to keep engines running cleaner. Older carbureted engines and farm equipment also lean on ethanol-heavy fuels for smoother operation and for cutting down air pollution. The U.S. Department of Energy reports that nearly all gasoline sold contains a measure of ethanol, helping reduce fossil fuel demand and greenhouse emissions. For me, living in the Midwest, towns rally around ethanol production—there’s more than a paycheck at stake; it’s a lifeline for local economies.
If you’ve swiped your face with toner, watched nail polish dry, or picked up a bottle of hand sanitizer, chances are acyclic alcohol played a big part. Ethanol acts as an antiseptic, sneaking into sprays and gels we count on to keep our hands bacteria-free. Isopropanol, another familiar face, stands out cleaning cuts and keeping wounds from getting worse. Everyday routines get a boost from these chemicals, and I trust the bottle in my cabinet because strict standards watch over their safety.
Factories, labs, and even repair shops lean on these alcohols to scrub surfaces, dissolve grease, and remove stubborn grime. Methanol works full-time as a solvent, helping engineers strip away residue or prep surfaces for fresh paint. It comes with risk—methanol can harm people if handled wrong, which highlights a need for good training and clear labeling at every workbench or mixing station. Industry groups advocate for strong oversight, and workers deserve to expect that when they reach for a bottle, it does the job without putting them in danger.
Acyclic alcohols help deliver medication in liquid form. Cough syrups, tinctures, and over-the-counter remedies often rely on ethanol as a carrier or preservative. Pharmaceutical labs trust these alcohols because they don’t just blend easily—they also fight off bacteria and extend a medicine’s shelf life. People tend to overlook these silent ingredients, but pharmacists and regulatory agencies keep close tabs to make sure products are both effective and safe.
Alcohols deliver value, but not every use comes without a tradeoff. Methanol, for example, costs lives if improperly stored or consumed. Accidental exposure, especially among kids or in places struggling with counterfeit spirits, creates tragedy far too often. Better packaging, tighter rules on labeling, and smart public health messages actually save lives. Cleaner engines and safer cleaning products start with better chemistry and clear regulations.From making transportation greener to filling first aid kits, acyclic alcohols prove usefulness time and again. By staying vigilant—with smarter packaging, regular testing, and honest discussion about risks—we get the benefits without so many of the downsides. Folks working in labs or fueling cars might not always think about it, but getting these basics right builds trust and keeps communities safe.
Acyclic alcohols show up in places most people don’t even realize. Ethanol, for example, forms the backbone of alcoholic drinks. Try buying cough syrup or cleaning products, and you’ll likely spot isopropanol on the label. What links these substances is their acyclic structure: a chain of carbon atoms, not a ring. Their safety depends entirely on which member of the alcohol family lands in our hands.
Read about methanol, and one learns of a tragic legacy—bootleg liquor and accidental poisonings. Methanol’s appeal vanishes quickly after the facts settle in. A tiny dose upwards of 10 mL can blind or kill an adult. The body processes it into formaldehyde and formic acid, and that’s where the danger comes from. Even simple skin contact, over time or in quantity, presents a genuine risk.
Ethanol stands on a different rung. It takes larger doses to produce harm—though it arrives stealthily. Excessive drinking can scar the liver for life. Still, ethanol is generally recognized as safe for consumption in modest volumes; regulators keep a close watch on what goes into the bottle.
Isopropanol makes its mark as a household disinfectant or hand sanitizer. People rarely drink it intentionally because the aftertaste is awful and the results, toxic. Medical staff rely on its rapid germ-killing power, but children, especially, need supervision. Ingesting even a small amount can bring on drowsiness, vomiting, or worse.
Regulators put clear-cut boundaries on alcohol use for a reason. Safety labels and warnings follow strict rules. Methanol never shows up in spirits or flavor extracts. Industrial alcohol producers often color it bright to keep drinkers away. Meanwhile, ethanol passes through tight controls before it gets close to a pharmacy or food processing site.
Handling, storage, and labeling work only if people read instructions and respect the risks. Safety data sheets spell out hazards for people working with acyclic alcohols in labs and factories. Modern guidelines go beyond simple use—transport, disposal, and spill cleanup protocols exist because a splash to the eye or skin can lead to trouble.
Accidents often begin at home, with containers left uncapped, or medicines within easy reach of children. The most effective solution means educating users, right where use actually happens. Labels only go so far if users brush them aside. Public health campaigns help push the message, but habits change slowly.
Technology lends a hand. Child-resistant caps, denatonium benzoate (to make products taste foul), and better packaging have cut down on accidental poisoning. Poison control centers spread the word even faster. Still, the most reliable gatekeeper is a street-smart approach: keep dangerous alcohols out of reach, locked away, and properly marked.
Basic chemistry doesn’t change, but the way society interacts with acyclic alcohols evolves. Knowing which molecules linger in the cupboard, which ones belong in the medicine cabinet, and which must stay in the garage keeps avoidable harm at bay.
Safety follows from understanding. Scientific research tests each acyclic alcohol for toxicity and long-term effects. Government agencies require rigorous studies, not just tradition, to set exposure limits and approve new uses. Mistakes, when they hit the news, often reveal the cost of cutting corners or skipping warnings.
People trust that the bottle from the pharmacy won’t hurt their family. That trust rests on a web of research, rules, clear labeling, and personal accountability. As society keeps learning, safer use follows—if everyone joins in.
Alcohols make it easy for us to get lost in jargon, but their core structure shapes everything from their smell to their role in industry. Acyclic alcohols carry a carbon chain without any loops. Think ethanol, found in drinks and hand sanitizer. Cyclic alcohols wrap those carbon atoms into a ring. Cyclohexanol stands out here. These two families don’t just differ in shape—their chemistry spins in separate directions.
Acyclic alcohols usually appear as straight or branched chains. Their hydroxyl group (-OH) sits along an open carbon skeleton. In the lab, those open ends make acyclic alcohols more predictable. They dissolve in water easily and often evaporate fast. Ethanol and methanol mix with water so well they disappear in a glass. This property also makes them handy for cleaning, fuels, and pharmaceuticals.
Cyclic alcohols, on the other hand, pull carbon into a circle. Their closed structure alters everything—from reactivity to strength. Cyclopentanol comes as a five-membered ring. Cyclohexanol bumps it up with six. These rings don’t just look different; they act different. Their molecules mesh in ways that change boiling points and melting points. For instance, cyclohexanol boils at about 161°C, which is much higher than ethanol’s 78°C. Tightly packed rings can’t escape into vapor as easily, so you need more heat. This makes cyclic alcohols suitable for things like plasticizers, perfumes, and even the synthesis of materials for car parts.
Every organic chemist learns to respect ring strain. Small cyclic alcohols, like cyclopropanol, hold their angle like a drawn bow, ready to snap. This stored energy means smaller rings often break open in reactions more easily than bigger, more stable rings. That doesn’t just fascinate in theory. In industry, it determines how these alcohols get used. A stable ring might serve as a base for medicines or coatings. Something prone to popping open can join in creative syntheses, like new drug molecules or adhesives.
Many acyclic alcohols, especially methanol and ethanol, show up all around us. They can become dangerous in the wrong doses. Methanol, for example, turns toxic quickly—ingestion can lead to blindness or worse. That’s a constant reminder that just because a molecule looks like something familiar doesn’t make it safe. Cyclic alcohols play a smaller but growing role in our lives. Cyclohexanol serves as a building block in making nylon, a fabric in almost every closet. Both groups have environmental footprints to consider. Large-scale production can create waste and require careful management of emissions. Recycling methods and green chemistry solutions—like enzyme-driven biosynthesis—keep working to improve that balance.
Smart chemistry makes life better. Engineers work on safer ways to make, use, and break down both acyclic and cyclic alcohols. Catalysts keep getting better for transforming these molecules with less waste. Teams study plant-based feedstocks to produce alcohols with less fossil fuel reliance. Even everyday people, by picking products that use less harmful solvents or more recycled content, join the push for safer, greener alcohols. Just as the shapes of these molecules differ, the direction of progress depends on how we use science to steer industry and everyday habits.
Acyclic alcohols, such as ethanol or propanol, are nothing new to anybody who's spent time in a chemistry lab. Still, the journey from textbook diagrams to large batches in factories offers lessons you won’t find on a classroom whiteboard. Take ethanol for example—its production scales from backyard fermentation to industrial plants churning out thousands of liters every day. People have made it for centuries by fermenting sugars with yeast. This age-old approach remains hard to beat for making drinkable spirits or biofuels. The reason? Nature designed yeast to do this job without complicated equipment or exotic chemicals. Toss in some corn or sugarcane, wait a few days, and you've got alcohol.
Look closer and you’ll spot plenty of science humming in the background. As demand for cleaner-burning fuels rose, so did the drive to wring more alcohol from less feedstock. Industrial producers optimize every batch—selecting fast-fermenting yeasts, balancing temperature, managing waste gases. Even slight tweaks in process can lift yield or purity, trimming costs without needing fancy tricks. Anyone who’s run a home-brew kit recognizes the instinct: if you can pull more value out of your setup, you do it.
Making acyclic alcohols isn’t just about food and drink. These compounds prop up chemical and pharmaceutical industries. To meet tougher demands—think higher purities or unusual chain lengths—the focus shifts from natural to synthetic chemistry. Take ethylene hydration for example. This process turns ethylene gas from petroleum cracking into ethanol. A catalyst, often phosphoric acid on a silica carrier, drives a reaction with water at elevated heat and pressure. Ethanol leaves the reactor, ready for further purification. No yeast, no sugar, and no waiting—just steam, pressure, and precise chemical control. This way, the industry can meet massive ethanol needs without raiding food supplies.
Longer-chain alcohols like propanol or butanol bring their own twists. Propanol springs from propene hydration—close cousin to ethylene hydration. Butanol production leans on the oxo process, coupling propylene, carbon monoxide, and hydrogen using metal catalysts to build the alcohol with fine control over structure. These synthetic methods crank out pure products at scale, keeping up with rising demand from solvents, fuels, or plastics.
Despite proven processes, trouble spots demand fresh thinking. Large-scale fermentation eats up farmland and uses fuel for distillation. Synthetic routes rely on oil or gas as feedstocks, locking the industry to fossil resources. And waste management, especially with some fermentation methods, can strain local ecosystems. It hits home in regions where factories sit close to farming communities, or where water runs short.
Researchers keep chipping away at those problems. Using waste cellulose instead of food crops for fermentation could slow the race between fuel and food. Green chemistry aims for new catalysts working at lower temperatures to cut energy bills. Even genetic engineering finds its place, building microbes that churn out alcohols from unusual or cheap wastes. Everyone who cares about cleaner energy or safer manufacturing should keep an eye on these advances, as they might unlock sustainable production without doubling costs or harming farmlands.
Each way to make acyclic alcohols comes from long learning—both on the lab bench and factory floor. Chemistry doesn’t offer shortcuts, but it does reward those who watch for better ideas and act on them. Whether for bottles, engines, or another feedstock, the story of acyclic alcohols blends science, practicality, and a sharp eye for what tomorrow might ask.
| Names | |
| Preferred IUPAC name | alkanol |
| Other names |
Propyl alcohol Isopropyl alcohol Butyl alcohol Isobutyl alcohol |
| Pronunciation | /ˈeɪ.saɪ.klɪk ˈæl.kə.hɒlz/ |
| Identifiers | |
| CAS Number | 64-17-5 |
| Beilstein Reference | 171 |
| ChEBI | CHEBI:23484 |
| ChEMBL | CHEMBL449108 |
| ChemSpider | 33131 |
| DrugBank | DB13879 |
| ECHA InfoCard | 100.029.289 |
| EC Number | 01.02.01 |
| Gmelin Reference | Gmelin Reference: 069872 |
| KEGG | C01103 |
| MeSH | D000355 |
| PubChem CID | 6857 |
| RTECS number | UC6050000 |
| UNII | 30SFG9737A |
| UN number | UN1987 |
| Properties | |
| Chemical formula | CnH2n+2O |
| Molar mass | 74.12 g/mol |
| Appearance | Colorless liquid or solid |
| Odor | alcoholic |
| Density | 0.81 g/cm³ |
| Solubility in water | Soluble in water |
| log P | 1.04 |
| Vapor pressure | 0.0208 mmHg at 25 °C |
| Acidity (pKa) | 16-18 |
| Basicity (pKb) | 13-15 |
| Magnetic susceptibility (χ) | -7.5 × 10⁻⁶ |
| Refractive index (nD) | 1.4100 |
| Viscosity | 0.59 mPa.s at 20°C |
| Dipole moment | 2.67 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 174.0 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -285.83 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -1368 to -3270 kJ·mol⁻¹ |
| Pharmacology | |
| ATC code | J05AB |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02, GHS07 |
| Signal word | Warning |
| Hazard statements | H226, H315, H319, H335 |
| Precautionary statements | P210, P233, P240, P241, P242, P243, P261, P271, P280, P303+P361+P353, P304+P340, P305+P351+P338, P312, P337+P313, P370+P378, P403+P235, P501 |
| NFPA 704 (fire diamond) | 2-3-1 |
| Flash point | 23°C |
| Autoignition temperature | 220–470 °C |
| Explosive limits | 3.3–19% |
| Lethal dose or concentration | LD50 oral, rat: 1870 mg/kg |
| LD50 (median dose) | 1,870 mg/kg (rat, oral) |
| NIOSH | NIOSH: UB7875000 |
| PEL (Permissible) | 100 ppm |
| REL (Recommended) | 240 |
| IDLH (Immediate danger) | IDLH: 2000 ppm |
| Related compounds | |
| Related compounds |
Acyclic ethers Acyclic hydrocarbons Aromatic alcohols Cyclic alcohols Diols Glycols |
