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2,2,3',3'-Tetramethylbutane emerged as an interesting branch in hydrocarbon chemistry during the early studies of branched alkanes. Back in the twentieth century, researchers were fascinated by the impact of extensive branching on both the physical behavior and reactivity of hydrocarbons. Understanding such a highly branched structure forced chemists to rethink how chain length and molecular shape influence boiling points, melting behavior, and interactions with different reagents. Over the decades, experiments involving this compound informed much of what we know about steric hindrance and the intricate nature of hydrocarbon rearrangement. Organic labs started using it as a reference for compactness in carbon skeletons, drawing on those historical experiments to set the groundwork for today’s synthesis and separation work.
2,2,3',3'-Tetramethylbutane shows up in labs as a clear, colorless liquid under standard conditions. With its heavily branched skeleton, this hydrocarbon grabs attention not just for its odd name but for how it bulks up without adding many carbon atoms. Chemists often point to it in discussions about the limits of carbon branching. In practical settings, you encounter it packaged in tightly sealed glassware or metal containers, kept away from moisture and ignition sources. Its purity tends to run over 98%, especially in analytical or synthetic work, highlighting a demand for minimal impurities to avoid side reactions.
One standout feature lies in its boiling and melting points. The heavy branching lowers these properties compared to its less-complicated relatives. This molecule resists freezing at the temperatures you’d expect from straight-chain butane, reflecting the challenges for its molecules to arrange neatly in any solid form. Its relatively low density often surprises those handling it for the first time. The molecule is non-polar, showing minimal solubility in water but blending easily with most organic solvents. Thanks to all this branching, you see less reactivity towards common oxidants and acids, offering some chemical stability even under heat.
Industry and laboratory labeling require precision. 2,2,3',3'-Tetramethylbutane features a CAS number (594-82-1) and a molecular formula C8H18. Technical sheets from manufacturers list its density around 0.764 g/cm³ at 20°C, boiling point near 106°C, with flash points generally under 10°C. Labels warn about the dangers of inhalation, flammability, and potential reactions with strong oxidants. Storage directions stress cool, ventilated conditions and the use of spark-proof tools. Regulatory compliance focuses on safety data sheets designed to help researchers spot hazards on sight, a critical step given volatile organics’ record in industrial settings.
Producing pure 2,2,3',3'-Tetramethylbutane starts from targeted alkylation. Lab syntheses often take a smaller alkane core, such as 2,3-dimethylbutane, and install extra methyl groups through reactions with methyl halides using strong bases or catalysts. Some routes have used Friedel–Crafts conditions, leaning on aluminum chloride to activate the hydrocarbons and attach those methyl branches. Controlling reaction temperature and stoichiometry means a cleaner yield with fewer over-alkylated byproducts. Once formed, distillation under reduced pressure or chromatography isolates the target molecule, giving chemists that signature compact, highly branched product.
The dense branching makes this molecule resilient in the face of aggressive chemistry. It resists oxidation, only slowly reacting with strong agents like potassium permanganate. Its inert nature toward acids and bases has made it valuable for testing apparatus or as a diluent in sensitive reaction schemes. Extreme heat or free-radical initiators can bust open its skeleton, but most functionalization attempts meet either total resistance or sluggish conversion, in part due to a lack of available hydrogen atoms on primary carbons. Because of this, modifications often focus on indirect strategies, such as generating derivatives through controlled chlorination or exploring its rare reactions for mechanistic studies.
In scientific circles, this molecule appears under several names: 2,2,3,3-Tetramethylbutane, Di-tert-butylmethane, and simply TMB. Suppliers list these names interchangeably, sometimes branding the compound based on purity, grade, or intended use. Knowing all variations becomes useful when sifting through chemical catalogs or product specification sheets, especially across different regions or regulatory environments.
Lab work with 2,2,3',3'-Tetramethylbutane requires robust safety protocols due to its flammability and potential respiratory hazards. Standard precautions involve working in fume hoods, using anti-static equipment, and storing the material in explosion-proof cabinets. Since its vapors start to build up at room temperature, air quality monitoring ensures concentrations don’t approach upper explosion limits. In case of spills or fire, teams carry dry powder extinguishers instead of water-based units, which risk spreading fires. Material Safety Data Sheets demand frequent review, calling out emergency procedures for skin or eye contact, as this hydrocarbon still carries typical risks found with volatile organics.
Uses for 2,2,3',3'-Tetramethylbutane highlight its chemical stability and unique structure. It serves as a calibration standard in gas chromatography, delivering consistent retention times without substrate interaction. The scientific community values it as a steric benchmark in molecular modeling and quantum chemical calculations, teaching about non-bonded interactions and spatial limits. Sometimes, makers of specialty fuels or lubricants use it to tweak combustion characteristics and viscosity, though the cost of synthesis keeps usage niche. I’ve seen it pop up in studies on isomer stability, giving researchers insight into why certain molecular frameworks favor energy minimization through branching.
Recent R&D efforts dig into the molecule’s role as a template for creating crowded environments in catalytic studies. Investigators look for catalysts that can shuffle carbon skeletons without breaking bonds indiscriminately, using 2,2,3',3'-Tetramethylbutane to test limits on reaction space. Advances in analytical chemistry have used it to probe interactions in gas-phase ion chemistry, tracking how higher-order hydrocarbons fragment under electron impact. Its performance as a reference in mass spectrometric methods remains steady. Researchers are also exploring innovative synthesis techniques to cut costs and reduce hazardous waste, aiming to broaden the field of hydrocarbon isomer research.
Studies on the toxicity of 2,2,3',3'-Tetramethylbutane suggest a low acute toxicity profile, based on animal studies and analogs in the hydrocarbon family. Still, inhalation can produce central nervous system effects, akin to other light alkanes. Chronic exposure data run thin, so handling guidelines stick to limiting duration and using personal protective equipment. Environmental fate studies point out sluggish biodegradation and a risk of bioaccumulation, especially if released into water systems. Regular review of new toxicology data matters, particularly as the molecule sees expanded lab use and new production methods bring potential impurities.
Expect growing interest in branched alkanes like 2,2,3',3'-Tetramethylbutane as tools for teaching molecular complexity and engineering reaction systems with built-in steric challenges. Green chemistry initiatives aim to refine synthesis protocols, looking for milder and safer reagents. As computational modeling grows, this molecule stands as a benchmark in simulations of hydrocarbon packing, steric effects, and energy landscapes. Improved accessibility and lower costs could let research labs expand practical study, while stricter environmental scrutiny will push for eco-friendlier synthesis and disposal methods. The next wave of innovation lies in coupling traditional hydrocarbon chemistry with bio-inspired catalytic strategies, using molecules like this one to test the outer edges of what’s possible—with safety, sustainability, and practical application in mind.
2,2,3',3'-Tetramethylbutane might seem like just another name buried in a long list of organic chemicals, yet this molecule draws the eye for a few solid reasons. It belongs to the alkane family, a group known for their stability. Unlike compounds that react at the drop of a hat, this one pretty much keeps to itself. Ask folks in organic chemistry labs, and most will tell you that such stable hydrocarbons pull their weight in research settings, especially where a chemical’s steady nature takes the stress out of sensitive experiments.
Labs often measure the strengths and weaknesses of various molecules. Here, chemists hunt for benchmarks—things that don’t react much, mess up results, or muddy the water. 2,2,3',3'-Tetramethylbutane fits the bill as a gold standard. It’s a hydrocarbon that refuses to play tricks. I’ve talked with analytical chemists who swear by this molecule for equipment calibration. It plays a role in calibrating gas chromatography machines, letting scientists determine how quickly different substances travel through a column. That means researchers get clearer snapshots of more unstable materials.
Anyone who’s studied organic chemistry has spent hours wrestling with how molecules bend, twist, and behave. 2,2,3',3'-Tetramethylbutane sports a compact structure, loaded with methyl groups, and shows extreme molecular crowding. Professors flag this molecule as a textbook example for students. Once, sitting in a university seminar, I remember an instructor pulling up its 3D structure to challenge the class: “Find something tighter packed,” he joked. It helps illustrate limits within chemical bonding. Besides education, computer models often compare new designs to this molecule given its pronounced bulk, which cannot be easily outdone.
I’ve noticed that thermodynamic researchers turn to this alkane when comparing experimental values to theoretical predictions. Because it resists reaction, measurements like boiling and melting points hit high accuracy. These data points anchor broader chemical studies by letting researchers double-check results against a reliable guidepost. Beyond theory, folks checking the purity of new hydrocarbon blends test their samples against well-known compounds like this one.
Unlike many hydrocarbons, 2,2,3',3'-Tetramethylbutane usually stays out of high-volume industrial streams. It avoids use in fuels or plastics for the simple reason—it’s not easy to make in bulk, and cheaper materials get the job done. Still, researchers don’t ignore safety. Alkane vapors, even low in reactivity, can catch fire under the right spark. Experienced hands always stress good ventilation and sealed containers.
Synthetic chemists like to throw puzzles at themselves. How much stress can a carbon skeleton handle before it caves in? This compact molecule stretches those limits. By examining its properties, teams have nudged the creation of even more crowded, intricate hydrocarbons. Sometimes, learning the edges of stability sparks new pathways in materials science or fuels design.
Few manufacturers supply 2,2,3',3'-Tetramethylbutane easily, which puts a cap on how widely it’s used. If labs or companies could boost supply with greener methods or lower costs, more researchers might put this molecule to work. I’ve met scientists eager for smaller alkanes with locked-in properties; outreach by specialty chemical firms could make those wishes reality.
High school chemistry left a mark on me. There’s no shortcut around getting your hands dirty drawing isomers, counting carbon atoms, and placing hydrogen atoms in their precise spots. 2,2,3',3'-Tetramethylbutane sounds like a mouthful, but it follows a logical pattern in organic chemistry. The base framework, butane, already gives four carbon atoms lined up. Adding tetramethyl means four extra methyl (–CH3) groups stick out from specific spots.
Let’s break it down. The first “2,2” means two methyl groups cling to the second carbon on the straight chain. The “3',3'” signals two more methyl groups fixed to another carbon, often on the opposite side for symmetry. Every time my fingers crept across a notepad, sketching out these branches, I learned to spot how bulkier molecules get with these extra methyls.
In chemical research, accuracy counts. If one carbon gets missed, the compound’s nature changes completely. Drawn with care, 2,2,3',3'-Tetramethylbutane totals out as eight carbon atoms, eighteen hydrogens: C8H18. That’s the same as the formula for octane. It startled me the first time I realized two very different-looking molecules could share a formula. Chemists call them structural isomers. This might seem academic, but it reminds us of the complexity hiding inside seemingly simple numbers.
I recall early laboratory days where figuring out these differences often meant the distinction between a successful reaction and something that fizzled out. Having C8H18 scrawled on a bottle label is not enough; shape and branching send ripple effects through reactivity, boiling point, and even the smell.
A molecular formula by itself doesn’t tell the whole story, but it does lay a foundation. In fuel chemistry, knowing C8H18 comes as octane and its relatives means understanding the backbone of gasoline. Tinkering with molecular shape—swapping straight chains for branched like in 2,2,3',3'-Tetramethylbutane—nudges up performance. Branched isomers typically help engines knock less, even with the same number of atoms.
During fieldwork for a local renewable energy startup, I saw up close how critical it was to recognize isomers. Blending fuels with the “right” version improved combustion, emitting less pollution and wasting less energy. It turns out that molecular structure reshapes real results, not just textbook problems.
Supporting a new generation of chemists means showing that formulas capture the outcome of years of measuring, drawing, and experimenting. Understanding a molecule like 2,2,3',3'-Tetramethylbutane requires patience and respect for detail. Focusing education and research on bridging the gap between formula and function could create safer fuels, smarter pharmaceuticals, and greener materials.
To make progress, investing both in basic chemistry training and in-demand laboratory tools pays off. Hands-on practice, not just memorization, let me see why getting every atom right matters. In my own work, revisiting the roots—structures and formulas—helped spark new ideas for more sustainable solutions.
Finding the molecular formula for 2,2,3',3'-Tetramethylbutane drew a line between abstract learning and practical action. The answer, C8H18, holds real value. There’s power in solid fundamentals and in asking hard questions about what’s behind every number.
2,2,3',3'-Tetramethylbutane doesn’t spark instant recognition for most people. It's a type of highly branched alkane, part of the hydrocarbon family found in fuels, solvents, lab reagents, and sometimes popping up in research. You won’t see it at the grocery store or a hardware shelf, but anyone working in chemistry or certain industries might have handled it.
For regular folks, running into this compound in everyday life is unlikely. It’s not tucked into cleaning sprays or slathered on crops. Lab workers, though, get a front-row seat. This stuff appears mainly in experiments aimed at understanding hydrocarbon structure and reactions.
Let’s cut through the jargon. 2,2,3',3'-Tetramethylbutane shares traits with other short-chain alkanes: it burns easily and vaporizes fast. Light a match anywhere near a vapor cloud, and flames will shoot up. It won’t corrode steel pipes or melt plastic bottles, but its real risk lies in fire hazards and the fact that breathing high concentrations can make you dizzy.
Safety authorities like OSHA and NIOSH don’t dedicate listings to this particular molecule. That’s not a free pass; it simply means research is limited. Data from similar hydrocarbons suggest that spills evaporate quickly, and inhaling concentrated fumes could leave someone gasping for fresh air, nursing a headache, or, in lousy ventilation, suffering from a lack of oxygen.
I’ve handled chemicals for years, and the basics never change: treat all unknown liquids and vapors as potentially risky. I’ve seen colleagues rush routines, confident they’ve seen it all, then stagger away coughing after a splash, or panic when a spark ignites vapors around a bench. Quick respect for a compound like 2,2,3',3'-tetramethylbutane saves you the drama. Keep it far from open flames, work in a fume hood, and cap containers the moment you’re done.
The compound evaporates quickly, rising up and dispersing into the air. Unlike some notorious hydrocarbons, it doesn't stick around in soil or water or build up in plants and animals. That sounds like good news, but high volumes dumped or spilled could stretch the limits of local air quality. Burning it pushes more carbon dioxide into the atmosphere, which, in small lab volumes, is barely a blip, but in the context of massive industrial use, these tiny impacts add up.
Chemical safety data sheets recommend a simple plan: gloves, goggles, and decent airflow. I don’t step into any chemical storage without a spill kit nearby. Fires need dry chemical extinguishers — not water, since vapor fires can flash fast across the surface. Repeat mistakes cost time and sometimes health, so drills and reviews for safe handling and quick cleanup matter more than fancy equipment.
This is a low-profile chemical, but industry and academia can’t ignore it. Assigning dedicated storage, clear labeling, and teaching proper handling protects both workers and resources. Most accidents stem from carelessness, not the substance itself. Emphasizing routine safety culture works better than fancy lockboxes or rare emergency protocols — especially with a compound as flammable as this.
Anyone who has handled specialty chemicals knows there is little room for error with substances like 2,2,3',3'-Tetramethylbutane. This compound’s molecular bulk and volatility mean little mistakes can turn into big accidents. My early years in a university research lab showed me more than a few close calls with organic solvents. Proper storage isn’t just a checklist item—it's about peace of mind when working late or sharing a bench with others. Getting it right keeps people safe and research on track.
This hydrocarbon looks harmless—clear, nonpolar, a faint gasoline smell—but it evaporates easily if left uncapped and catches fire in the sort of air everybody breathes. Flammability sits at the top of concerns. I’ve seen colleagues store less volatile substances far from heat or sparks without thinking twice; with tetramethylbutane, that diligence pays off in accident-free labs.
Every class in chemical safety drills a few simple truths. Keep flammable liquids away from direct sunlight, ignition sources, and places prone to sudden temperature spikes. Always seal containers tight. My own preference has always been amber glass bottles with PTFE-lined caps. These containers don’t react with nonpolar organics and block ultraviolet light, which adds a layer of protection. Fact: hydrocarbons degrade faster in bright light, and leaky lids lead to fumes and contamination. A shelf with proper ventilation and temperature control—ideally, under 25°C—pays dividends over time. I once saw a plastic-capped bottle swell and crack during an August heatwave; we spent hours dealing with fumes that a glass bottle could have handled.
No one grabs a bottle labeled only “organic compound X” in a pinch. Good habits keep everyone on the same page, which is crucial in group settings where sleep-deprived grad students juggle a dozen side projects. Every bottle should carry a clear hazard label, name, and acquisition date. Group similar volatile organics together, but always separate them from oxidizers, acids, and bases. I once returned from conference travel to find a careless mistake—an oxidizer stored next to several flammables—and it could have ended with a call to the fire department. Segregation helps prevent incidents others pay the price for.
Open a volatile hydrocarbon outside designated fume hoods and you’ll smell it in seconds. That’s your nose warning you about vapor exposure. Flammable liquid cabinets with forced ventilation pull those fumes outside, keeping working air safer. If budget limits access to expensive cabinets, storing the chemical away from traffic, or in secondary containment trays, adds a meaningful margin of safety.
Spill kits—absorbent pads, sand, inert barriers—should always sit nearby. Early in my career, a seasoned technician showed me how quickly spills spread, and how fast prompt containment heads off panic and expensive cleanup. If everyone knows the drill, small leaks stay small.
Hydrocarbons build up degradation products or container residues. A best practice involves tracking purchase dates and using older material first. I keep logs updated to avoid surprises when an impurity ruins a week’s work, or the safety team pops in for a surprise check and asks about the faded bottle at the back of the cabinet. Routine disposal keeps chemicals from lingering past their prime and triggering headaches with compliance or safety.
2,2,3',3'-Tetramethylbutane sounds like a mouthful. In the lab, this molecule gets some attention for its structure. Built from a straight butane backbone, the carbon atoms branch at just the right spots, tacking on extra methyl groups (CH3) at positions two and three. These extra methyls turn butane’s already simple chain into something bulkier, a true isomer standout.
Anyone who has worked with branched alkanes knows the story changes as you move from a linear layout to something more congested. In this compound’s case, those methyls prevent close packing, which affects melting and boiling. While n-butane starts vaporizing below room temperature, 2,2,3',3'-Tetramethylbutane clings stubbornly to its solid form unless you heat things up to around 100°C (212°F), a vivid jump way above the parent molecule. If you’ve ever pulled this off a shelf expecting just another volatile gas, the high melting point makes it memorable.
It won’t dissolve in water. No surprise there. The molecule releases any hint of polarity and slides easily into nonpolar solvents like hexane or ether. Spilling a few milligrams on the bench only leaves behind a faint chemical scent and nothing sticky—tell-tale signs it won’t bind with water or stick to glassware for long.
Folks in research meet this molecule while testing theories about steric hindrance. Take it from anyone who’s puzzled over a failed reaction: too many methyls clustered together can block reactants from coming close. This bulky nature turns the molecule into both a tool and a troubleshooting nightmare, testing patience and glassware as you try to coax it into dissolving or reacting.
Because natural gas and gasoline rely on how molecules stack together, 2,2,3',3'-Tetramethylbutane helps illustrate some big-picture ideas. Bulky molecules resist easy combustion; they burn cleaner than long, straight chains. For those watching smoky exhausts or tinkering with fuel efficiency standards, understanding these properties shapes conversations on cleaner fuels.
Students dragging themselves through organic chemistry labs come away remembering just how odd solid alkanes look at room temperature. It’s not like pulling a block of paraffin from a candle—tetramethylbutane is crystal clear, waxy, and out of place beside the oils and fluids that dominate most benchtops.
Outside the classroom, this chemical doesn’t wind up in common products. It’s too specialized and finicky. But its properties tell a broader story about how changing a structure impacts what we see and handle. Anyone who’s added a few methyl groups to tune flavor molecules, scents, or pharmaceuticals knows the smallest tweaks can turn a watery liquid into a slow-melting solid.
The world needs chemists who get why structure matters. For safer handling, stockrooms should keep this molecule sealed tight and labeled clearly, since anyone expecting a liquid can end up with a clogged pipette. Manufacturers on the scale-up side can look to this as a model when designing new, stable chemicals for storage and shipment. In every case, small changes inside the molecule shift how we work with the material—as much as the eye can see and as much as the hand can feel.
| Names | |
| Preferred IUPAC name | 2,2,3,3-Tetramethylbutane |
| Other names |
Hexamethylethane Tetramethylbutane 2,2,3,3-Tetramethylbutane |
| Pronunciation | /ˈtuː tuː θriː θriː ˈtɛtrəˌmɛθəlˌbjuːteɪn/ |
| Identifiers | |
| CAS Number | 594-76-3 |
| 3D model (JSmol) | `JSME 2.7.6 2 2 4 C 1.0 0.0 C 2.2 1.3 C 3.4 0.0 C 4.6 1.3 1 2 1 1 3 1 2 4 1 1 1 1 1 3 1 1 4 1 1 1 1 1 1 4` |
| Beilstein Reference | 3918731 |
| ChEBI | CHEBI:141561 |
| ChEMBL | CHEMBL15457 |
| ChemSpider | 60751 |
| DrugBank | DB14130 |
| ECHA InfoCard | ECMC: 100.124.669 |
| EC Number | 203-650-7 |
| Gmelin Reference | 62170 |
| KEGG | C06585 |
| MeSH | D015407 |
| PubChem CID | 11227 |
| RTECS number | EL8575000 |
| UNII | 56V9A1X1CS |
| UN number | UN1208 |
| CompTox Dashboard (EPA) | DTXSID7048974 |
| Properties | |
| Chemical formula | C8H18 |
| Molar mass | 114.23 g/mol |
| Appearance | Colorless liquid |
| Odor | Gasoline-like odor |
| Density | 0.792 g/cm³ |
| Solubility in water | Insoluble |
| log P | 2.6 |
| Vapor pressure | 5.43 kPa (at 20 °C) |
| Acidity (pKa) | pKa ≈ 50 |
| Basicity (pKb) | Product 2,2,3,3'-Tetramethylbutane does not have a pKb value because it is a hydrocarbon and does not exhibit basicity. |
| Magnetic susceptibility (χ) | -75.8·10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.3827 |
| Viscosity | 0.674 mPa·s (20 °C) |
| Dipole moment | 0.0 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 289.0 J⋅mol⁻¹⋅K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -177.8 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | –6587 kJ·mol⁻¹ |
| Hazards | |
| Pictograms | GHS02,GHS07 |
| Signal word | Warning |
| Hazard statements | H225, H304, H336, H411 |
| Precautionary statements | Keep away from heat, hot surfaces, sparks, open flames and other ignition sources. No smoking. Store in a well-ventilated place. Keep cool. Wear protective gloves/eye protection/face protection. |
| NFPA 704 (fire diamond) | 1-4-0 |
| Flash point | 71 °F |
| Autoignition temperature | 415 °C |
| Explosive limits | 0.9–7% |
| Lethal dose or concentration | LD50 (oral, rat): >5 g/kg |
| NIOSH | RN1404 |
| PEL (Permissible) | PEL: Not established |
| REL (Recommended) | 1000 ppm |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
Isobutane Neopentane Hexane 2,2-Dimethylbutane 3,3-Dimethylpentane |
