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Chemistry has a long tradition of diving deep into the world of hydrocarbons. 2,3-Dimethylbutane stood out for scientists in the early twentieth century, not for its fancy applications but because it brought much-needed clarity to the study of molecular structures and the concept of isomerism. That's the puzzle where compounds build from the same number of carbons and hydrogens yet show up with different personalities. 2,3-Dimethylbutane, a branched alkane, highlights how even tiny tweaks in carbon chain branches spin off entirely new possibilities in chemical behavior. Textbooks favored it: students learned what a difference methyl groups at carbon 2 and carbon 3 could make, compared to the simple, straight-chain hexanes. As time rolled forward, this hydrocarbon claimed its place as a go-to model for teaching and for testing refinements in organic synthesis. Where research into fuel chemistry or cracking processes happened, you’d find 2,3-Dimethylbutane lurking in the background, providing benchmarks and control samples to check theories against.
2,3-Dimethylbutane presents itself as a clear, colorless liquid at room temperature with a typical hydrocarbon odor that never fails to remind you of fueling stations and the sharp tang of solvents. It may sound like just another member of the alkane crowd, but its branched structure gives it a few tricks. Chemists often reach for it to illustrate how branching influences boiling points and reactivity—2,3-Dimethylbutane boils at a lower temperature than unbranched hexane, which might seem counterintuitive until you dig into the science. Its primary appeal comes through as a reference liquid in the study of gasoline composition, octane ratings, and the hunt for fuel blends that resist engine knocking. People don't really see it in stores or buy it as a consumer good—its role stays behind the scenes, serving professionals in research, refining, and industrial settings.
This molecule, with its six carbons and two methyl groups branching from the main line, gets counted in the family of C6H14 isomers. Its boiling point slides in below that of many straight-chain alkanes—around 58°C, lighter on its feet than its cousin n-hexane, which boils closer to 69°C. Physical properties tell a lot about safety and storage. It floats on water, barely dissolves, and vaporizes easily enough to demand respect from anyone handling it. Being nonpolar and less reactive than alkenes or aromatics, it prefers sitting out of the most dramatic chemical reactions unless heat or a strong spark shows up. Its stability owes a lot to those extra methyl branches that make the molecule compact.
Laboratory bottles always mark 2,3-Dimethylbutane clearly. I’ve seen “2,3-Dimethylbutane,” “dimethylethylmethane,” and sometimes a synonym like “biisopropyl.” Labels indicate flammability first and foremost, as this liquid catches fire easily. Good practice requires a tightly sealed container, kept away from ignition sources, and no mixing it near oxidizing acids or peroxides. Many labs tuck it into lockers rated for Class 3 flammables, as required under chemical safety codes. MSDS sheets flag its tendency to give off flammable vapors even at fairly cool temperatures. No dye, no odd color, no perfume—it’s all about transparency and precaution.
2,3-Dimethylbutane can trace its synthesis to classic organic lab work. Refiners isolate it from certain petroleum fractions through precise distillation, but bench chemists sometimes build it from scratch. A common route involves alkylation of isobutane with isobutene, catalyzed by strong acids like sulfuric acid or hydrofluoric acid. This pathway doesn’t just spit out 2,3-Dimethylbutane by itself; other branched alkanes show up too, so purification, through fractional distillation or selective adsorption, steps in next. This process mimics what happens during the catalytic reforming of gasoline—an industrial process designed to bump up the octane rating by making more branched molecules like this one. The simplicity of the molecule means that, industrially, large-scale separation from natural sources beats out elaborate chemical synthesis. Still, the chemistry behind its preparation remains a staple in the training of organic chemists looking to understand hydrocarbon transformations and separation techniques.
This hydrocarbon keeps a low profile in terms of reactivity, which is typical for alkanes. Without double bonds or exposed functional groups, 2,3-Dimethylbutane resists reaction unless strong conditions enter the picture. Free radical halogenation—think chlorine or bromine in bright light—turns it into a wild mix of mono- and poly-halogenated products. High temperatures or catalytic conditions break it apart in cracking processes, trimming down those six carbons or rearranging the skeleton. In fuel studies, researchers feed it through reforming reactors, tweaking operating conditions to see how quickly it reshuffles into aromatics or other high-octane components. If you try oxidizing it, don’t expect much beyond a messy collection of carbon oxides and water, unless precise control and selective catalysts earn their keep.
Open up a chemistry database or a supplies catalog, and you may run into alternative names for 2,3-Dimethylbutane. Its main synonyms include “diisopropyl,” based on its two isopropyl groups, and “biisopropyl.” The IUPAC name leaves no ambiguity: 2,3-Dimethylbutane. Literature sometimes abbreviates it to “2,3-DMB,” especially in technical discussions about gasoline isomers. All refer to the same colorless, flammable liquid with a structure confirmed by X-ray crystallography and NMR decades ago. For clarity, professional circles prefer the IUPAC version unless space is tight or shorthand is the order of the day.
Every professional who’s worked with flammable chemicals has a safety story, often involving “simple” alkanes like 2,3-Dimethylbutane. Flammable liquids demand caution, especially those with low flash points—this molecule will ignite from a spark at roughly -19°C, posing serious risks in labs and storage facilities. Best practices call for well-ventilated spaces, explosion-proof refrigeration, fire extinguishers at arm’s reach, and personal protective equipment such as goggles and nitrile gloves. Facilities handling 2,3-Dimethylbutane often draft strict protocols for storage, transfer, and spill cleanup, shaped by guidelines from bodies like OSHA or local fire authorities. The liquid’s volatility means ordinary air movement can build up enough vapor to reach the lower explosive limit, making routine checks and reliable ventilation systems a must. Over time, I’ve seen labs run drills, review procedures, and invest in vapor detectors, treating even seemingly “harmless” alkanes with respect they’ve always deserved.
Even though 2,3-Dimethylbutane rarely finds its way into household or retail products, it plays an outsized role in industries where the nuances of fuel behavior matter. Its status as a reference isomer puts it on the front line of octane number testing, industry research into knocking resistance, and refining process optimizations. By mapping how blends respond in engines, petrochemical engineers seek to squeeze out higher performance and efficiency. Some specialty fields, such as analytical chemistry, use this compound as a retention time marker in gas chromatography, anchoring measurements of unknowns against well-defined standards. Environmental scientists pay attention, too, analyzing traces of 2,3-Dimethylbutane and its isomers when tracing pollution from fuel leaks or spills. This molecule’s behind-the-scenes influence stretches from labs and refineries all the way to the highways, quietly shaping the gas in countless car tanks.
There’s always something new to learn from simple hydrocarbons. For years, research with 2,3-Dimethylbutane has centered on fuel science, engine design, and the search for higher-octane blends that burn clean yet pack plenty of energy. Graduate students often start out by studying the boiling points or vapor pressures of this molecule, updating charts used in the design of fuel systems. In refinery R&D, engineers test catalysts that rearrange hydrocarbon mixtures, watching how quickly 2,3-Dimethylbutane breaks down or morphs into more valuable fragments. Analytical chemists calibrate instruments with this compound, confident that its known properties will anchor other measurements. On the synthetic front, interest in branched alkanes never fades: researchers explore greener processes to produce or separate these molecules with less waste or lower energy demands, taking cues from trends in “sustainable chemistry.” Mapping the fate of 2,3-Dimethylbutane in environmental samples after spills or incomplete combustion builds data sets for future regulations and remediation efforts.
Most people assume the smaller alkanes pose little risk beyond fire hazards, but any volatile organic compound deserves closer examination. Research on 2,3-Dimethylbutane’s toxicity points to a low level of acute toxicity—exposure to vapors in poorly ventilated spaces can induce headaches, dizziness, or nausea. Chronic exposure, as with many hydrocarbons, raises questions about potential impacts on the nervous system and other organs, though this risk remains far lower compared to aromatic compounds. Its low solubility in water lessens the risk of groundwater contamination, but inhalation or accidental ingestion demands quick medical response due to the potential for aspiration and chemical pneumonitis. Regulatory agencies place tight limits on permissible workplace exposure, and anyone handling this compound gets the usual reminders: good ventilation, never work alone, and know the route to the nearest eyewash station or emergency shower. Toxicology labs continue to refine testing, sometimes using animal models to trace long-term organ effects, building a stronger evidence base for health protections.
As the world trends toward cleaner fuels, tighter safety rules, and deeper environmental scrutiny, the profile of 2,3-Dimethylbutane may shift. Its stability and clear behavior as a marker compound will sustain its role as a research tool and a quality standard in the energy sector. Advances in catalysis could unlock more selective production routes, cutting down on waste during fuel blending or reforming. Growing interest in alternative fuels and stricter air quality standards might push the need for this molecule as a calibration standard in emissions testing, tracing volatile hydrocarbons with ever-greater precision. On the safety front, better sensors and handling protocols promise to lower incident rates wherever this compound appears. And teaching labs won’t let go of 2,3-Dimethylbutane anytime soon—the lessons it offers on branching, reactivity, and chemical safety remain as direct and relevant as ever, both for new generations of chemists and those already deep in the industrial world. Whether in refining, research, or regulation, this modest hydrocarbon will keep earning its place on the shelf.
2,3-Dimethylbutane doesn’t show up in glossy ads or consumer product labels. That doesn’t mean it sits forgotten. Folks working behind the scenes—fuel chemists, research lab techs, and chemical engineers—know this hydrocarbon by heart. To many, it's just one of several isomers in the family tree of hexane. Its everyday impact stems from much more than textbook chemistry.
One common place to spot 2,3-dimethylbutane is the petrol and fuels business. This colorless liquid shows up as a standard among reference fuels used in engine testing. Researchers depend on it to check knock resistance, or octane rating, which basically measures how smoothly fuel burns inside an engine. Automakers want to iron out engine knock since it ruins efficiency and causes long-term wear. By mixing known amounts of 2,3-dimethylbutane with similar molecules, testers create blends with very specific combustion traits. This way, they can match, score, and improve real-world fuels for modern engines.
I’ve seen how even small changes in chemistry shift gas performance. In one project, a little more branched hydrocarbon like 2,3-dimethylbutane made a surprising difference in both knock-prevention and engine temperature. That kind of control helps companies reach cleaner emissions and better fuel economy—two targets that aren’t going away.
Lab students and seasoned chemists also cross paths with 2,3-dimethylbutane during synthesis work. It's not a headline-making feedstock, but it does challenge the basics of molecular structure. In organic chemistry courses and research, tackling the rearrangement, cracking, or isomerization of such compounds often acts as a jumping-off point. Students learn how subtle shifts change physical and chemical behavior. Researchers use it to test out new catalysts or to map out reaction pathways, which sometimes leads to discoveries in petroleum processing or green chemistry.
There’s something grounding about hands-on experiments with simple hydrocarbons. In undergraduate labs, the unmistakable smell of compounds like 2,3-dimethylbutane lingers long after glassware is clean. You see molecular theory come to life—and realize why some compounds become teaching standards.
Not everything about this compound is positive. Like other light hydrocarbons, 2,3-dimethylbutane brings health and flammability risks. Many safety data sheets warn about inhalation hazards and the danger of fires, and people in labs or industry can’t afford to skip protective gear or precautions. Compared to some older, more harmful solvents, branched alkanes like this one are less toxic, but safe handling remains a real lesson.
Factories and universities have started looking for safer or renewable ways to achieve the same end results. Some research groups are investigating bio-based or less volatile molecules to use in solvent applications and testing. Regulatory agencies, including the EPA, pay close attention to volatile organic compounds in the air and their role in smog formation. That scrutiny pushes companies and academic labs to question each product’s full life cycle.
The real value of 2,3-dimethylbutane lies in these intersections—energy, safety, education, and innovation. Single compounds like this shape broader trends in energy, science learning, and safer workspaces. Rather than focus on glamour or household visibility, the workhorse role proves just as vital. Big-picture improvements in fuel quality, cleaner air, and smarter chemical design all have roots in small molecules and everyday lab lessons.
2,3-Dimethylbutane belongs to the family of alkanes, which means its foundation lies in simple carbon and hydrogen bonds. Its structure forms a branched arrangement. There’s a straight four-carbon backbone with methyl groups attached at the second and third carbon positions. This gives it the formula C6H14. Looking at a ball-and-stick model in an organic chemistry lab, you’ll notice how those branches open up space, shaking up its physical characteristics compared to a straight-chained relative like n-hexane.
Pour a bit of 2,3-Dimethylbutane into a beaker and raise the heat. This compound boils at roughly 58°C (136°F), so it doesn’t take much energy to push it from liquid to vapor. The melting point hovers around -128°C (-198°F). For those working with low-temperature environments, this low melting point really matters because it remains a liquid long after water or even ethanol has frozen solid.
Clear, colorless, and with a faint, gasoline-like odor, you’d have a hard time telling 2,3-Dimethylbutane apart from other similar alkanes just by looking or sniffing. Having handled chemicals like this in the lab, it’s always a surprise how something so unassuming can wind up as a central piece in fuel research or process engineering – a reminder to respect those obscure flasks and bottles.
With a density of almost 0.66 g/cm³ at 20°C, this molecule floats nicely above water. During experiments or accidental spills, it forms a slick, glimmering layer on top. Trying to dissolve it in water proves a frustrating exercise; as an alkane, it resists mixing. This low solubility comes from its nonpolar bonds that simply don’t play well with the polar nature of water. On the flipside, 2,3-Dimethylbutane blends with other organic solvents like diethyl ether or hexane, making it handy when crafting chemical cocktails for organic reactions.
On a warm day, 2,3-Dimethylbutane wants out of its bottle. It evaporates quickly, thanks to a vapor pressure at 20°C of about 340 mmHg. I’ve learned that labs with poor ventilation can rapidly fill with the odor of evaporating hydrocarbons, underscoring the importance of working under a fume hood, not just to keep things tidy, but to dodge serious health risks.
This molecule lights up fast, with a flash point at a chilly -22°C (-8°F). Applying basic lab safety here isn’t just a checklist item. Back in college, a fellow student learned the hard way that a Bunsen burner left a bit too close to a hydrocarbon sample results in a fireball and a stern talking-to from the supervisor. Proper storage – tightly sealed containers, no open flames, and good airflow – keeps everyone safe and headaches to a minimum.
Most people never come face-to-face with pure 2,3-Dimethylbutane. It slips into gasoline blends to improve combustion and can find a spot as a standard in analytical chemistry. There’s an ongoing conversation about alternatives to volatile hydrocarbons to ease pressure on air quality and reduce risks both in industry and research. Exploring safer, greener solvents stands out as a promising direction. Conversations in lab teams and industry panels keep circling back to ways of reducing exposure, boosting containment, and strengthening training for those handling chemicals. Chemical literacy, clear labeling, and regular safety drills make a world of difference – not just for the specialists, but for anyone sharing a workspace or community with these hidden yet powerful molecules.
2,3-Dimethylbutane doesn’t turn many heads unless you work in a lab or a refinery. This hydrocarbon shows up as a clear liquid with a faint gasoline smell. You’ll spot it in fuel blends or research settings, but it hasn’t found its way into everyday home products or foods. What’s its risk to your health? The answer depends on how and where you encounter it.
Most people relate chemical danger to skin burns or toxic fumes that make you cough or worse. 2,3-Dimethylbutane belongs to a class of compounds known as alkanes, close chemical cousins to components in gasoline and lighter fluid. They’re flammable and volatile. Breathing in high concentrations, like in a room with poor ventilation, brings on dizziness, headache, and fatigue. These aren’t friendly symptoms at all. At higher doses, unconsciousness or fatal respiratory depression can happen — like with other hydrocarbon fumes.
Anyone working with this chemical needs to take fire safety seriously. 2,3-Dimethylbutane vapors catch fire fast. Static sparks or open flames can set off a blaze before you notice anything’s wrong. I’ve experienced chemical storage rooms where the smell alone warned of trouble — the air felt charged, every movement deliberate, everyone careful not to surprise the fumes. Emergency safety kits and constant air checks became second nature.
Letting hydrocarbons slip into soil or water doesn’t just ruin a day. It threatens wildlife and drinking water sources. 2,3-Dimethylbutane doesn’t break down quickly outside, so a spill lingers. Small creatures and fish find these chemicals especially nasty. Some studies suggest persistent hydrocarbon pollution can cause birth defects or immune system failures in aquatic life. Preventing leaks isn’t just a box-ticking exercise; clean water and healthy soil depend on real containment practices.
Most exposure risks show up during industrial work. Refinery staff, lab technicians, or transportation crews handle this liquid daily. Spills can soak skin or splash eyes, both painful and a fast way for trouble to start. Home exposure almost never happens, but car repair or mismanaged fuel storage could bring an unlucky person close. Inhalation of fumes remains the real threat.
The European Chemicals Agency and the US Occupational Safety and Health Administration both classify alkanes like 2,3-Dimethylbutane as dangerous because of their ability to harm lungs and nervous systems, and start fires. No one recommends exposure limits higher than a few hundred parts per million for short periods. Most guidance calls for gloves, goggles, and strong ventilation as the frontline defense.
My experience in industrial settings hammered home one thing: planning beats panic every time. Facilities that train workers, invest in ventilation systems, and prioritize regular safety reviews rarely see accidents. Signs, spill kits, and clear emergency exits aren't luxuries, they’re the best tools against injury or harm.
For industries handling chemicals like this one, safer transport containers and better leak detection systems really make a difference. Research keeps pushing toward green chemistry, aiming for fuels and solvents that don’t carry the level of risk seen in volatile hydrocarbons.
2,3-Dimethylbutane poses real risks when handled carelessly, but with the right preparation and respect for its fire and toxicity hazards, harm can be kept at bay. Experts, regulators, and workers share the responsibility to keep exposure controlled and the environment protected.
Chemistry doesn’t always have to mean staring at incomprehensible symbols or memorizing strange names. Take 2,3-Dimethylbutane as an example. It stands out as an isomer of hexane, with the chemical formula C6H14. Anyone who has poked around in an organic chemistry textbook will instantly spot that familiar formula. But the difference comes down to how the atoms connect—a detail that shapes everything from a molecule’s physical properties to its real-world uses.
Picture the standard butane backbone: four carbon atoms joined in a straight chain. With 2,3-Dimethylbutane, two methyl groups (–CH3) slip onto the second and third carbons. Now, the basic chain doesn't run straight any longer. The skeletal formula turns into:
CH3-CH(CH3)-CH(CH3)-CH3
Here, each “branch” plays a role in the molecule's behavior. The structure can also be written as:
C6H14
or drawn for clarity as:
CH3 CH3 | |CH3–C–C–CH3 | | CH3 CH3
That branching turns 2,3-Dimethylbutane into something special. Compared with straight-chain hexane, it evaporates faster and lights up more easily. These quirks arise from the way branching influences both surface area and how tightly molecules pack together. In gasoline production, 2,3-Dimethylbutane's high octane rating makes it a valuable tool for reducing engine knock. That means less pinging under the hood, a smoother ride, and even a boost in fuel efficiency.
Every molecular fork in the road creates new possibilities. Working in a high school lab years ago, I watched as a teacher poured samples of various hexane isomers into test tubes. The more branches appeared on a molecule, the lower its boiling point dropped. That stuck with me. It showed, in a straightforward way, how a simple shift in structure leads to new applications—from solvents in industry to blending components in fuels.
Handling 2,3-Dimethylbutane requires care, just like other hydrocarbons in its class. It burns with a clean flame yet produces carbon dioxide and water, along with the risk of harmful emissions in confined spaces. Preventing spills and leaks, using suitable ventilation, and keeping the material away from open flames are basic but essential. Students and professionals alike must learn safe handling not only by reading data sheets but by paying attention every time they work.
The conversation with hydrocarbons keeps circling back to sustainable development. Improving refining methods, searching for alternatives, and investing in cleaner engines can reduce the environmental footprint of molecules like 2,3-Dimethylbutane. Education shouldn’t stop at knowing structures. Promoting a shift toward renewables not only helps communities but steers the conversation to a healthier relationship with our planet.
Storing and handling chemicals in the lab or industrial setting often means building routines that go deeper than just rules on a label. 2,3-Dimethylbutane, a colorless, flammable liquid, has earned a reputation for lighting up too easily and letting off fumes that can sneak up and cause trouble. With a low flash point, the stuff goes up fast if there’s a stray spark or a forgotten open flame. Folks who work with volatile organics know from experience—one distracting conversation or worn-out piece of equipment can be all it takes to put people and property at risk.
Metal safety cans and explosion-proof storage cabinets always seem like overkill until that close call actually happens. A chemical like this belongs in a sturdy, airtight container that has no cracks, no chance for accidental leaks. My experience tells me to look for containers with a good seal but without complicated valves that somebody might forget to shut tight. Flammable liquid safety cabinets, the yellow ones with fire-resistant walls, provide a real barrier if something goes wrong. I learned early on to keep the cabinet clean—wiping up drips, and making sure nothing collects inside that could start a fire.
Heat and sunlight turn these liquids tricky, especially in older buildings where the ventilation can be less than perfect. Storing 2,3-Dimethylbutane away from direct sunlight, heaters, and electrical panels pays off. Lab managers really see the gaps on the hottest summer days. Most folks set the cabinet in a cool, dry part of the workspace, away from windows and airflow that can push vapors toward ignition sources. Using a flammable-rated refrigerator helps if the chemical needs to stay chill, but a household fridge, with its switches and light bulbs, creates more danger than it solves.
Carrying out transfers and pouring from bottles calls for eye protection and solvent-resistant gloves. Splash-proof goggles keep the eyes safe from any surprise slosh. I always grab a lab coat, and a lot of people add a face shield if there’s a chance of big splashes. Working over trays or absorbent mats catches spills before they slide off the workbench. Veteran techs insist on grounding everything—whether it’s a metal drum, a portable pump, or a transfer line. Static electricity surprises nobody more than the person pouring from one container to another.
An overlooked step comes in how much 2,3-Dimethylbutane folks leave sitting around. Smaller, well-labeled containers keep the work careful. Only pulling out as much as the job needs means less to clean up if an accident happens. Someone once told me, “Don’t tempt fate with a bigger mess than you feel like cleaning.” That stuck.
Vapors can drift, build up, and flash over if people ignore airflow. Good labs rely on proper ventilation, like fume hoods or local exhausts, so that workers aren’t breathing in hydrocarbons day after day. Air monitors—simple units that beep if concentration goes above safe levels—let workers relax a bit, knowing a silent problem won’t linger undetected. In bigger spaces, open doors or windows alone rarely cut it. Mechanical help, like fans made for hazardous locations, keeps the air moving and safe.
Even the most careful worker spills now and then. Emergency procedures, practiced ahead of time, form the difference between a hassle and a disaster. Absorbent material, spill kits, and fire extinguishers rated for flammable liquids belong nearby. Everyone on the crew should know who to call and what steps come next if something goes wrong. Regular training sessions, including fire drills, put muscle memory in place so panic doesn’t win out. In my experience, a confident, well-practiced response brings down the risk during a bad moment.
Experience shapes safe work. Labels fade, containers change, but habits built on routine care and clear training endure. Chemical safety doesn’t spring from fear; it grows from respect for the tools and chemicals at hand, and from a willingness to challenge shortcuts or unsafe practices before they take root. Keeping that mindset saves real headaches, real costs, and lives.
| Names | |
| Preferred IUPAC name | 2,3-Dimethylbutane |
| Other names |
Diisopropyl 2,3-Dimethybutane |
| Pronunciation | /ˌtuːˌθriː-daɪˈmɛθɪlˌbjuːteɪn/ |
| Identifiers | |
| CAS Number | 79-29-8 |
| Beilstein Reference | 1718733 |
| ChEBI | CHEBI:88364 |
| ChEMBL | CHEMBL140742 |
| ChemSpider | 6828 |
| DrugBank | DB01971 |
| ECHA InfoCard | 100.116.399 |
| EC Number | 203-613-9 |
| Gmelin Reference | 1076 |
| KEGG | C06535 |
| MeSH | D016689 |
| PubChem CID | 6566 |
| RTECS number | EI8575000 |
| UNII | PVT6U269JF |
| UN number | UN2351 |
| Properties | |
| Chemical formula | C6H14 |
| Molar mass | 86.18 g/mol |
| Appearance | Colorless liquid |
| Odor | gasoline-like |
| Density | 0.653 g/cm³ |
| Solubility in water | insoluble |
| log P | 2.82 |
| Vapor pressure | 53.32 kPa (at 20 °C) |
| Acidity (pKa) | Acidity (pKa) of 2,3-Dimethylbutane: 50 |
| Magnetic susceptibility (χ) | -68.4·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.384 |
| Viscosity | 0.406 mPa·s |
| Dipole moment | 0.00 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 229.2 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -167.0 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | –3896 kJ·mol⁻¹ |
| Hazards | |
| GHS labelling | No GHS labelling. |
| Pictograms | `GHS02` |
| Signal word | Warning |
| Precautionary statements | P210, P261, P271, P304+P340, P312, P403 |
| NFPA 704 (fire diamond) | 1-1-0 |
| Flash point | -25 °C |
| Autoignition temperature | ~365 °C (689 °F; 638 K) |
| Explosive limits | 1.1-7.5% |
| Lethal dose or concentration | LD50 (oral, rat): 4,000 mg/kg |
| LD50 (median dose) | LD50 (median dose): 5000 mg/kg (rat, oral) |
| NIOSH | NA1117 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) for 2,3-Dimethylbutane: Not established |
| REL (Recommended) | 200-1000 |
| IDLH (Immediate danger) | IDLH: 900 ppm |
| Related compounds | |
| Related compounds |
2-Methylpentane 3-Methylpentane n-Hexane 2,2-Dimethylbutane |
