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In the early 20th century, chemists began isolating and studying individual hydrocarbon compounds, such as 1,4-pentadiene, as part of the larger effort to understand unsaturated chemical structures. Laboratories across Europe and North America recognized the potential locked in conjugated and isolated double bonds, given their unique reactivity and possible uses in synthesizing polymers, pharmaceuticals, and agrochemicals. During the prolific post-war era of chemical innovation, industrial researchers tuned their focus onto these five-carbon dienes, refining distillation, purification, and storage techniques to keep the unstable compound from polymerizing or reacting with oxygen. Sulfur or hydroquinone stabilizers became industry standards, allowing safe transportation and storage on larger scales. My own work with older chemical catalogs from the mid-20th century always shows notes about stabilization, reflecting the lessons learned through decades of trial, error, and sometimes, disaster.
1,4-Pentadiene, sold in stabilized forms to prevent unwanted reactions, stands out as a linear hydrocarbon with two terminal double bonds. As an intermediate, this compound carves out a niche in chemical manufacturing, serving as a backbone for further synthesis in industries that need reactive olefins. Chemical suppliers package it in stabilized forms, usually with small amounts of antioxidant, to curb peroxide formation and uncontrolled chain reactions. Engineers and chemists working on specialty polymers prize this diene for its role in cyclization, cross-linking, and as a stepping stone to more complex molecules. During my graduate research in a polymer chemistry lab, I saw firsthand how a small vial of 1,4-pentadiene, handled with respect and kept under inert gas, can open doors to novel materials, creative linkers, and intriguing small molecule libraries.
At room temperature, 1,4-pentadiene appears as a clear, colorless liquid with a distinct hydrocarbon odor. Its boiling point sits around 42 to 44 degrees Celsius, making it quite volatile, and the compound evaporates quickly if left to the open air. The density is lower than water—about 0.68 g/cm³—so spills float and spread easily. Its solubility profile places it firmly among nonpolar substances; it lifts out of organic solvents such as hexane, benzene, or toluene, but resists mixing with water. The real story lies in its chemical makeup: terminal double bonds at the 1 and 4 positions provide plenty of opportunities for addition reactions, polymerization, and cycloadditions. These properties draw researchers and process chemists time and again, looking to harness the reactivity for creative syntheses or clever new materials.
A bottle of 1,4-pentadiene from a reputable supplier usually arrives marked with CAS number 592-95-0, along with hazard designations reflecting its flammability and reactivity. Technical data sheets include measured purity, usually in the high 90% range, and stabilize concentration—often less than 200 ppm of hydroquinone or a similar agent. Chemists delve into the technical notes to check for residual water content, unsaturated impurity levels, and acceptable storage conditions (cool, dry, under nitrogen atmosphere). Regulatory compliance and standardized hazard pictograms stem from lessons learned through industry mishaps, and those familiar red skirts and flame icons on the label act as a daily reminder that this isn’t a molecule you leave uncapped at the bench. In my own practice, strict adherence to labeling springs not just from legal obligation, but respect for my mentors’ cautionary tales—of ruined syntheses, lab evacuations, or fires sparked by ignored warnings.
Production of 1,4-pentadiene usually relies on elimination strategies, where a suitable precursor such as 1,4-dihalopentane undergoes dehydrohalogenation with a strong base. Sometimes, catalytic dehydrogenation of cyclopentene or cyclopentadiene offers an alternative, especially at scale. Industrial chemists watch temperature, catalyst selection, and reaction atmosphere closely, since even small deviations can tip the balance from productive yields to intractable byproducts or dangerous side reactions. Techniques such as fractional distillation, washing, and immediate stabilization with hydroquinone or sulfur become standard. Those in smaller-scale labs might turn to sodium amide or other strong bases, prepared with caution under inert conditions, to avoid runaway polymerization or noxious off-gassing. In every context I’ve experienced, the take-home lesson remains the same: speed, vigilance, and strict oxygen exclusion carry the day, whether the aim is a research sample or a ton for industrial processing.
The business end of 1,4-pentadiene centers on its terminal double bonds, which open doors to a raft of transformations. The diene system readily participates in Diels-Alder reactions, offering a path to cyclohexene derivatives when exposed to suitable dienophiles. Hydrohalogenation, hydration, hydroboration, and ozonolysis all reshape the molecule in well-studied, often selective ways, providing gluons for building more complex organic frameworks. In polymer chemistry, these double bonds permit controlled cross-linking and graphene-like structure formation under free-radical or cationic conditions. I’ve lost track of how many times I’ve encountered 1,4-pentadiene in retrosynthetic analyses drawn on whiteboards, the two pi bonds serving as modular handles for almost any synthetic ambition—if only one commands the instabilities with care.
In scientific and industrial circles, 1,4-pentadiene appears under a handful of names: penta-1,4-diene, sym-pentadiene, or simply, divinylmethane. Databases such as PubChem, ChemSpider, and REAXYS all cross-list these terms, ensuring that researchers across disciplines land on the intended compound. Commercial bottles sometimes carry the stabilization method in the name, such as “1,4-Pentadiene, stabilized with hydroquinone.” This diversity in terminology can trip up inexperienced chemists during literature reviews or ordering. In my collaborations with international partners, cross-checking synonyms on shipment paperwork has prevented supply chain snags and expensive misorders. It’s worth taking the few extra minutes, every time, to verify the product matches the research need.
Work with 1,4-pentadiene demands real vigilance due to its volatility and tendency toward spontaneous polymerization or violent ignition if exposed to heat, spark, or sunlight. Splash goggles, gloves, and flame-resistant lab coats count as baseline protection; chemical fume hoods and proper grounded storage vessels form another layer of defense. Emergency procedures hinge on containment, ventilation, and rapid reaction spill kits—no one takes shortcuts with this diene. Environmental regulations around volatile organic compounds touch every stage from shipment to disposal, and chemical hygiene plans spell out steps for reactive or exothermic decompositions. In my time running training sessions for new lab members, walk-throughs around flammable storage cabinets and hands-on review of MSDS sheets make sure nothing escapes notice. Every incident on record—be it spill, fire, or unwanted polymerization—began with “just for a moment” or “just this once.” Respect saves lives.
Polymer research, organic synthesis, agrochemical design, and even flavor and fragrance chemistry all dip into the well of 1,4-pentadiene at one point or another. In polymer science, the unique placement of the double bonds enables production of advanced copolymers, impact-resistant rubbers, and specialty resins. Organic chemists pull it into the fold for cyclization and cross-linking studies, while agrochemical scientists build more potent pesticides and herbicides from diene scaffolds. The flavor and fragrance sector, always on the hunt for new volatile backbones, experiments with 1,4-pentadiene derivatives to unlock green, earthy notes. As a graduate student working on new elastomer formulations, testing, tweaking, and sometimes cursing 1,4-pentadiene’s fickle reactivity became a staple in pushing product performance beyond what standard monomers could offer. Diverse applications spring from a single capability: raw, accessible reactivity that never sits still.
Current R&D efforts look at greener synthesis routes for 1,4-pentadiene, aiming to cut down on energy-heavy dehydrohalogenation and to swap out harsh reagents for milder, more sustainable catalysts. Academic labs explore harnessing biocatalysts or engineered microbes, viewing this diene as a platform chemical for more eco-friendly processes. Analytical chemists keep refining purification and detection techniques, focusing on trace impurity management, which can make or break downstream synthesis. In material science, research pivots toward designing new thermosets, adhesives, and coatings with better weathering and aging profiles, for which 1,4-pentadiene serves as a cross-linking agent. In my own consulting work with startup material companies, I’ve seen real investment flowing into safer stabilization, smarter containers, and digital monitoring of storage conditions—reflecting a realization that chemistry doesn’t just happen in glassware, but across shipping lanes and global supply chains.
Toxicological studies show that exposure to 1,4-pentadiene vapors can irritate the eyes, nose, and throat, with high concentrations posing risk of drowsiness or even asphyxiation in unventilated spaces. Animal studies report central nervous system effects at significant exposure levels. Chronic toxicity remains less well-characterized, but the compound's potent reactivity points toward potential for cell membrane disruption or genotoxic effects if mishandled. Among my colleagues in industrial hygiene, air monitoring and strict ventilation routines always accompany operations where this diene is in play. Regulatory reviews urge keeping exposure as low as reasonably achievable. Nurses and doctors in occupational clinics keep close watch for signs of accidental overexposures among chemical workers, acknowledging that safety protocols carry real, not just bureaucratic, weight.
Over the coming years, growth in advanced materials, green chemistry, and custom chemical synthesis looks set to fuel fresh interest in 1,4-pentadiene. The race for lighter, tougher, and smarter polymers unearths new uses for well-worn reactants like this diene, nudging the market toward smarter stabilization and modular production plants. Expect to see more focus on renewable feedstocks, digital process monitoring for safer scale-up, and data-driven risk management. Startups and established players alike invest in R&D that pushes synthesis beyond old limitations, testing new catalysts, automation-friendly purification techniques, and closed-loop recycling. Having worked on both bench chemistry and business strategy, I appreciate how technological momentum doesn’t just chase cost savings, but answers rising expectations for safety, sustainability, and high performance. The story of 1,4-pentadiene, far from over, keeps evolving right alongside the science that shapes tomorrow’s industry.
Most people never think about the hard science behind products that show up in daily life. 1,4-Pentadiene [Stabilized] shows up behind the scenes as a building block for synthetic chemistry. Its structure, with two double bonds, lays the groundwork for all sorts of reactions. I’ve spent time around chemists who appreciate simple molecules like this, not because of how they look, but because of what they can do.
It turns out that 1,4-Pentadiene serves as a foundation for making specialty polymers and resins. These are the kinds of materials that end up shaping the plastic parts in gadgets, the coatings on cars, and even the glue that sticks different components together. Chemists work with this compound because it allows for chain reactions, literally piecing together carbon atoms like beads on a string. This quality lands it a spot in many research and production labs where new materials get tested every day.
1,4-Pentadiene doesn’t like to sit still. Without a stabilizer, it can start reacting with oxygen or other chemicals in the air. Manufacturers add stabilizers so the compound doesn’t spoil before it’s put to use. Think of it as adding a preservative to bread so it lasts longer. This lets researchers and companies store and transport the chemical safely, reducing the risk of dangerous reactions. Having worked in environments where safety means everything, I know people rely on these kinds of precautions to keep projects moving smoothly.
Most organic chemists reach for 1,4-Pentadiene when crafting complex molecules. The dual double bonds act as a springboard. Through reactions like cycloadditions or cross-linking, this molecule helps construct rings or connect small units into long, sturdy chains. Sometimes, it gets used to make flavors, fragrances, and even pharmaceuticals. It helps add carbon skeletons needed for drugs or specialty aromatics. I’ve read patents that credit this molecule for breakthroughs in rubber compounding and fuel additives.
Safety isn’t just about keeping the compound bottled up. Handling 1,4-Pentadiene [Stabilized] calls for attention to ventilation and personal protective gear. Breathing in its fumes or letting it touch skin could cause harm. Regulations ask companies to limit worker exposure and manage waste materials properly. The chemical doesn’t stick around forever in the environment, but good practices lower the risk for people and ecosystems.
Seeing how green chemistry is gaining traction, some researchers look for ways to replace or recycle solvents and intermediates wherever possible. Companies often adopt closed systems and improved filtration to keep these chemicals contained and the workplace safer.
The conversation about 1,4-Pentadiene isn’t just about chemistry or production. It circles around training, transparency, and technical support. Training matters most—giving chemists, warehouse staff, and shippers the knowledge they need to manage chemicals safely. Tools like safety data sheets and regular audits help keep mistakes in check. On top of that, continued innovation makes it possible to use less hazardous stabilizers or design new processes that lower waste. It’s one thing to handle a powerful compound safely; it’s another to always seek smarter, greener methods as technology progresses.
The truth about 1,4-Pentadiene (Stabilized) doesn’t jump out at you until you’ve worked with it. My time in a university lab taught me a lot about respect—especially for volatiles like this. A slip in judgment or a shortcut can turn an ordinary day upside down. The odorous, clear liquid is both flammable and reactive. Crew in shipping warehouses and lab managers rarely forget the point: mishandling chemicals is not a matter of inconvenience; it’s one of safety—or, sometimes, life and death.
Let’s clear up a widespread assumption: stabilization prevents accidents, but it’s not the end of the story. Safety takes shape in the details. Temperature swings or drafty storerooms can undo all that extra care manufacturers put into the product. I remember one winter in the lab, pipes froze, and the temperature dropped well below the recommended 2–8°C range. The tension rose just thinking about what could happen. Some folks believe a shelf in a fume hood seals the deal—but open containers and air exposure present a constant risk for peroxides or unwanted reactions.
Heat brings more than discomfort in chemical storage. 1,4-Pentadiene evaporates easily and catches fire fast. My chemistry professor liked to say, “Hot room, short career.” Secure this stuff in a dedicated flammables cabinet, well away from sunlight or warm spots—never next to radiators, water pipes, or anything that puts off heat. Flammable storage cabinets aren’t overkill; they’re insurance.
Nothing sours a mood faster than opening a cabinet and finding a transfer bottle without a label. Original containers—those you get from trusted suppliers—offer more than a nice look. They use materials tested for this compound’s quirks, often polyfluorinated or glass, with tight-fitting caps to block air and minimize leaks. Resist the urge to repurpose even “clean” glassware; cross-contamination sits waiting for that one lazy moment.
Complacency grows quickly. You look at the same bottle for weeks and its hazards fade into the background. Real incidents—fires, unexplained pressure build-up, or skin burns—hit hardest on routines gone sloppy. Good storage practices lay the groundwork for a safer environment. Use secondary containment trays. Always mark the purchase and opening date right on the label so you’re not left guessing how old the stock is during inventory sweeps. Ventilation isn’t optional. Even stabilized stocks can emit vapors if a cap loosens or temperature rises. Fume hoods do the heavy lifting for air flow, catching accidents before they spiral.
Experience keeps bad habits at bay. I’ve seen how regular safety checks and peer reminders shut down carelessness before it spreads. Train everyone who enters your space. Don’t waste the lessons learned from someone else’s close call. It takes a few minutes to double-check all flammables at the end of a shift; it could take days or weeks to recover after a mishap. Attention to storage isn’t just a box to tick—it's an act of respect for everyone working nearby.
Working in a chemical lab brings back memories of handling dozens of compounds, each one with its own set of challenges. 1,4-Pentadiene stands out because its reactivity can surprise anyone who isn’t careful. This compound easily vaporizes, and its fumes catch fire quickly. So if you treat it like other organics and skip a few steps, you’re setting up trouble.
Most accidents happen when people skip gloves, goggles, or lab coats. I’ve seen lab mates splash solvents on themselves and rely on luck. Skin contact with 1,4-Pentadiene can burn or irritate, and eye exposure is far worse. Splash-proof goggles and gloves (nitrile or other chemical-resistant materials) keep the liquid and vapor at bay. A flame-resistant lab coat shields against the worst-case scenario—a chemical fire.
Ventilation makes a huge difference. Fume hoods aren’t for show. I once ran a chromatographic separation where someone ignored the hood, and for hours the whole area smelled like sweet gasoline. That’s a sign of vapor build-up, and one spark in that air would have caused disaster. Always carry out all work in a well-ventilated fume hood designed for flammable chemicals.
Most people overlook proper storage until something spills. 1,4-Pentadiene should go in tightly sealed containers, away from heat sources, direct sunlight, or oxidizers. Locking storage cabinets rated for flammable substances keeps the inventory organized and limits access. Clear labeling helps others know what they're grabbing—no one enjoys scrambling after a mystery leak.
Stabilizers slow down unwanted reactions, but they don’t turn 1,4-Pentadiene into a toy. Some colleagues assumed stabilized meant safe, but the risk of explosion and fire remains. If the stabilizer stops working, the compound can polymerize or ignite. That’s why date-checking, proper rotation, and not exceeding shelf-life help avoid old, unstable chemicals sitting forgotten on a shelf.
Sparks and static can trigger a fire in seconds. Grounding and bonding containers during transfers avoid unwanted static buildup. Keeping a proper fire extinguisher (foam or dry chemical) close by turns a scary moment into just another safety drill. For spills, inert absorbent materials lock down the spread, and ventilating the space keeps fumes low. Deactivation requires disposal under hazardous waste protocols, not a regular dumpster. Knowing emergency numbers and procedures by heart isn't just a safety box to check—it counts when seconds matter.
Most problems boil down to training and diligence. Every person who walks into a shared lab space should know standard operating procedures inside out. I remember a time in grad school a new intern skipped the chemical safety basics. Within days, they mixed incompatible solvents, risking a fire. Regular safety refreshers, visible signage, and a culture of peer checks work better than any rule book.
Chemicals like 1,4-Pentadiene serve plenty of useful purposes in synthesis and industry, but sloppy shortcuts stack up to serious risks. Relying on proper storage, tight safety gear, clear procedures, and team vigilance isn’t just compliance—it means everyone gets to finish the job in one piece.
For years, people working with solvents and industrial chemicals look out for more than a fancy molecular structure. They keep their eyes on danger warnings and flammability labels. 1,4-Pentadiene, even when labeled as “stabilized,” isn’t a sleepy bystander in the chemical warehouse. This stuff flashes off at a temperature you’d easily see in an everyday kitchen. Its flash point hangs at -27°C. There’s no need for a spark if a room heats up more than a winter’s day.
Run a search through chemical safety sheets and you see 1,4-pentadiene at the top of the flammable category. Fire codes in labs and manufacturing floors don’t make exceptions for “stabilized.” Once vapors get moving, a tiny spark or static charge can ignite a room. This isn’t mythology from anxious safety officers — case reports detail burns, evacuations, and flash fires.
A few years back, a lab in the Midwest nearly lost its roof during an experiment that used 1,4-pentadiene. The chemical had been properly stabilized, but fumes built up around faulty ventilation. The air mixture reached a point where a wayward electrical arc did the rest. Quick thinking with a fire extinguisher kept things from getting worse, but nobody chalked the event up to mere bad luck. Even stabilized, this chemical can make ordinary tasks dangerous.
Rows of bottles with clear liquids might look similar, but toxicology profiles quickly separate the dangerous from the benign. 1,4-pentadiene carries a strong, pungent smell. Inhalation isn’t something you shake off with a glass of water and a break outside. Exposure headaches, dizziness, and in severe cases, respiratory distress. Gloves and goggles can slow down accidental exposure, but common sense keeps people furthest from trouble.
Workers know from experience that a slip while decanting or a crack in a storage bottle leads to headaches that last days. The substance dries the skin and sticks to mucous membranes. During warmer months, vapors don’t just drift toward open windows; they settle, seeping into every corner unless fans run full tilt.
Daily life with 1,4-pentadiene means heavy reliance on explosion-proof refrigerators and double-sealed containers. The chemical doesn’t take kindly to sunbeams through a window, hot equipment, or even nearby heaters. Ventilated storage rooms tell a story: layers of warning stickers, cabinets locked tight, logs tracking every tiny amount that comes or goes.
I once spent a summer working inventory for an industrial supplier. Bottles of stabilized 1,4-pentadiene always meant careful moves, two people on every transfer, and an eye on temperature reminders. Even short lapses in storage habits invite trouble, especially on hot days.
Substitution ranks high on the wish list. Labs and production engineers look for alternatives with higher flash points and lower volatility. Until that’s possible, real solutions involve airtight facilities, proper sensors for vapor build-up, and relentless training. Automatic fire suppression systems and constant air quality checks cost money, but one accident wipes out every saving.
Digital logs and real-time alerts improve safety. Companies invest in training because nothing matches firsthand experience in keeping people healthy around such chemicals. Accidents shrink once everyone respects the threat and keeps to the letter of proven handling methods.
Anyone who spends time with 1,4-pentadiene can’t afford to ignore warnings. Flammable, no matter how well stabilized, means never letting your guard down. Upgraded systems and respect for safety keep stories about this chemical from turning into headlines.
1,4-Pentadiene comes up every so often in the world of organic chemistry, especially in laboratories where folks want to experiment with small-chain hydrocarbons. This molecule earns its name from its backbone—five carbon atoms hooked together like a short chain, with two double bonds inside. Unlike more complicated compounds, this one keeps its story simple: five carbons, a couple of double bonds, lots of odd uses in industry and research labs.
You spot the formula by counting atoms: C5H8. The structure spreads out with carbon atoms in a row, each labeled from one to five. The double bonds slot in at positions one and four, so you have those distinct unsaturations that make pentadiene much more than a boring alkane.
Draw it out and it looks like this:
CH2=CH–CH2–CH=CH2
This zigzag shows two alkenes right near each end of the chain. All that squeeze on carbon’s bonding means extra reactivity, and that matters outside the classroom too.
Straight from the bottle, 1,4-pentadiene doesn’t like to behave. As someone who’s handled flammable organics, you can see how a diene like this can cause headaches. Left unstabilized, those double bonds encourage reactions that form polymers or other unwanted byproducts. Pour a little stabilizer into the storage drum—typically something like butylated hydroxytoluene (BHT)—and reports of sticky gunk at the bottom of your flask start to disappear.
I’ve seen labs toss out expensive stocks because the chemical got too wild and polymerized after sitting around for a few months. Adding stabilizer right away stops headaches before they start.
Having those double bonds at either end opens up a handful of applications. Industries sometimes tap 1,4-pentadiene for synthetic work, especially when assembling longer, more complex molecules. Those extra electrons in the double bonds mean 1,4-pentadiene can act as a building block for various organic syntheses, especially in pharmaceutical or materials development. If you’re planning a Diels-Alder reaction, this molecule might be your star ingredient.
It’s important to point out the real safety concerns, too. That C5H8 formula translates to a low flash point and a vapor that can float through a busy lab. Some researchers set up proper hoods and invest in explosion-proof storage. Sticking with strict safety rules always beats cleaning up after a fire. Stabilization only does so much; smart handling finishes the job.
If chemical supply outfits adopt sealed ampoules and alarmed storage lockers, it cuts down on loss and risk. Some teams build automated monitoring to track purity and flag any hint of unwanted reactions. And nothing beats a fresh supply—ordering in small batches keeps both costs and hazards manageable. Simple, steady habits mean 1,4-pentadiene stays useful instead of annoying.
In the end, a simple structure like C5H8 brings both power and potential frustration. Keeping it stable, stored right, and only taking what’s needed helps researchers, students, and manufacturers keep their focus where it matters—on discovery, invention, and safe progress.
| Names | |
| Preferred IUPAC name | penta-1,4-diene |
| Other names |
Piperylene 1,4-Pentadiene, stabilized Divinylmethane UN 2044 |
| Pronunciation | /ˌwʌn.fɔːrˈpɛn.təˌdaɪ.iːn/ |
| Identifiers | |
| CAS Number | 2004-70-8 |
| Beilstein Reference | 1209245 |
| ChEBI | CHEBI:51308 |
| ChEMBL | CHEMBL503775 |
| ChemSpider | 68269 |
| DrugBank | DB13870 |
| ECHA InfoCard | 03b8c4a4-a6d6-4408-acee-b8c8862d4c04 |
| EC Number | 203-807-8 |
| Gmelin Reference | 148198 |
| KEGG | C02533 |
| MeSH | D017382 |
| PubChem CID | 11577 |
| RTECS number | SQ9275000 |
| UNII | 84X5B8NZ1N |
| UN number | UN2048 |
| Properties | |
| Chemical formula | C5H8 |
| Molar mass | 68.12 g/mol |
| Appearance | Colorless liquid |
| Odor | Gasoline-like |
| Density | 0.675 g/mL at 25 °C (lit.) |
| Solubility in water | Insoluble |
| log P | 1.94 |
| Vapor pressure | 17 mmHg (20°C) |
| Acidity (pKa) | 36.1 |
| Magnetic susceptibility (χ) | -10.5 × 10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.406 |
| Viscosity | 0.58 cP (20°C) |
| Dipole moment | 0.40 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 327.59 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | 84.4 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | 3246.6 kJ/mol |
| Pharmacology | |
| ATC code | V03AB37 |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02,GHS07 |
| Signal word | Warning |
| Hazard statements | H226,H304,H315,H335,H336,H411 |
| Precautionary statements | P210, P233, P240, P241, P242, P243, P261, P271, P280, P301+P310, P303+P361+P353, P304+P340, P305+P351+P338, P312, P337+P313, P370+P378, P403+P235, P405, P501 |
| NFPA 704 (fire diamond) | 2-4-2 |
| Flash point | 40 °F (USCG) |
| Autoignition temperature | 220 °C |
| Explosive limits | Lower 1.4%, Upper 8.6% |
| Lethal dose or concentration | LD50 oral rat 4600 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral-rat LD50: 3280 mg/kg |
| NIOSH | BZI61250 |
| PEL (Permissible) | Not established |
| REL (Recommended) | REL (Recommended): 0.1 ppm (0.35 mg/m³) |
| IDLH (Immediate danger) | IDLH: 1,000 ppm |
| Related compounds | |
| Related compounds |
1,3-Pentadiene 1,4-Hexadiene 1,5-Hexadiene 2,4-Hexadiene Cyclopentene |
