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Chemistry advances one compound at a time, often on the back of curiosity and a drive to solve practical problems. Decades past, the emergence of substituted diphenylmethanones like 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone signaled a shift in the way chemists approached molecular design. Research during the late 20th century revealed that manipulating aromatic rings with halogen and alkoxy groups could help fine-tune electronic and steric effects. This strategy opened paths toward active pharmaceutical intermediates and specialty materials, giving industrial chemists new levers to pull. As regulations around PCBs, DDTs, and other persistent halogenated compounds became stricter, the fine chemicals industry sought out molecules that offered performance without such legacy baggage. Chemists looked for selective reactivity, improved yields, and greater control over byproducts, and discoveries in diphenylmethanone derivatives fit these criteria.
5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone sits among a class of benzophenone derivatives with carefully chosen substituents. Its structure blends a bromine atom, a chlorine atom, and an ethoxy group scattered across the aromatic cores. These substitutions aren't chosen on a whim. For chemists designing this molecule, every group alters reactivity, solubility, and handling in concrete ways. I’ve seen product datasheets present this compound as a fine crystalline solid, marketed toward specialist labs and institutions working on the synthesis of high-value chemicals. Each batch’s consistency and purity can make the difference between a successful synthesis and wasted resources. Procurement teams scan its technical certificate for moisture content, melting point, and HPLC purity, because tight material specs prevent surprises at the bench.
This compound comes in as a white to pale yellow crystalline solid, often forming robust needles or plates that pack efficiently. Its molecular formula, C15H12BrClO2, yields a molecular weight of around 340.6 g/mol. Bromine and chlorine together grant a higher density and a higher boiling point compared to unsubstituted analogues. I have noticed that the electron-withdrawing nature of halogens mostly suppresses unwanted side reactions, providing an advantage during scale-up. Its melting point generally sits between 105°C and 109°C, a useful window that keeps thermal degradation risks low during purification. Ethoxy substitution slightly boosts solubility in organic solvents. You'll probably want to keep it dry—excess moisture risks hydrolysis or product caking, which can complicate both weighing and transfer. Halogenated aromatics can prove stubborn in water, but common organic solvents such as dichloromethane, acetone, and ethyl acetate dissolve it readily, allowing for flexible processing choices.
Anyone accustomed to regulatory compliance takes technical labeling seriously. For 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone, the certificate of analysis tells most of the story: purity regularly exceeds 98% by HPLC, and maximum allowable moisture hovers around 0.5%. Impurity profiles list residual starting materials and any by-products, an essential measure for customers who can't tolerate unknown peaks in final products. Tech sheets specify batch numbers, production dates, recommended storage temperatures (2–8°C), and shelf life, often two to three years under sealed conditions. Labels warn about halogen content, indicating risks if combined with strong bases or reducing agents. For those shipping outside Asia, UN classification and REACH registration become part of the sticker, supporting cross-border transport needs and regulatory needs in Europe and the United States.
Lab notebooks from organic synthesis classes usually begin with stepwise routes outlining how to build up substituted benzophenones. One standard method starts from a substituted benzoyl chloride—say, 5-bromo-2-chlorobenzoyl chloride—reacted with a para-ethoxylated benzene in the presence of AlCl3 or another Friedel–Crafts catalyst. The reaction, carried out under anhydrous conditions, typically proceeds with slow addition to control exotherms and maximize yield. Aqueous workup strips out catalysts and hydrolyzes intermediates, leaving an organic layer that crystallizes on standing. For multi-kilogram scale, process chemists invest in temperature-controlled reactors, continuous extraction, and inline analytics to catch faults before crystallization. Further purification may require recrystallization or column chromatography, especially for pharmaceutical intermediates where impurity thresholds fall below 0.2%.
Chemists value this compound for its stability alongside its flexibility. That bromo and chloro pattern opens doors to further coupling reactions. Suzuki-Miyaura and Buchwald–Hartwig couplings thrive here, as the aryl bromide reacts with boronic acids or amines to bolt on a new aryl or alkyl group where you want it. If you have experience with library synthesis for medicinal chemistry, you know these tools allow for rapid iteration on aromatic frameworks. The ethoxy group, less reactive under mild conditions, can be swapped for other alkoxy chains with more energetic conditions. Nucleophilic aromatic substitution can occur at the halogen positions, leading to amines or thiols. That flexibility supports its adoption in combinatorial screening, dye development, advanced materials chemistry, and as a handle for isotope labeling in tracer studies.
Walk into any reference library or database, and you’ll find a string of labels for this molecule. Some researchers refer to it as 5-Bromo-2-chloro-4’-ethoxybenzophenone. Catalog suppliers might shorten it to BCEDPM or give catalog-specific codes like “BE-402” to help procurement officers match order sheets with previous inventory. Larger manufacturers use internal batch codes and registration numbers that tie back to documentation and compliance records. A few entries in ChemSpider and PubChem document similar variations, each mapped to the same CAS number, helping to cross-check sources and ensure the correct compound enters the supply chain. For international customers, translations of names and precise stereochemistry avoid regulatory pitfalls and mislabeling.
Handling aromatic halogenated ketones means respecting both chemical and occupational health standards. Even experienced lab staff wear gloves, goggles, and lab coats when weighing, dissolving, or transferring this molecule. SDS documentation cautions against inhalation of dust, skin contact, and getting residues in eyes. Fume hoods prove essential for open transfers to limit vapor exposure, and any scale-up effort includes spill trays and emergency eyewash access. Disposal routes require special attention. Companies must collect and store spent solutions for disposal as halogenated organic waste, with strict documentation for shipment to licensed destruction facilities. Companies that have faced regulatory scrutiny over improper halogen disposal know that controls and staff training prevent future liability. Emergency protocols for spills or exposures stay posted in every prep room, as do instructions for first aid and who to call for help.
Industry and academia harness substituted benzophenones for much more than their direct uses. Medicinal chemists use them as building blocks for anti-inflammatory or anti-tumor compounds, especially when halogen and alkoxy arrangement alters binding affinity or metabolic profile. Materials scientists working on UV-cure coatings or specialty resins count on the ultraviolet-absorbing abilities of such ketones, since the right substitution can extend absorption deep into the near-UV. Agrochemical developers build libraries of analogues, searching for candidates with improved resistance to photodegradation in field environments. Polymer chemists exploit their cross-linking potential, enabling high-performance films or adhesives. In my own time working with CROs, the adaptability of this backbone gave both flexibility in project goals and a sense of direction, knowing that a single molecule can connect so many chemical worlds.
R&D efforts around these molecules focus on efficiency and lowered environmental impact. New catalytic methodologies and greener solvents dominate contemporary literature. Teams race to replace legacy Friedel–Crafts protocols with milder, recyclable alternatives, like organocatalysis or enzyme-based modifications. Automated synthesis modules and process monitoring now help chemists optimize reactions in real time, teasing out gains in selectivity or yield that batch recipes couldn’t provide. I’ve seen interdisciplinary groups use computational modeling to predict modifications’ effects before committing to long weeks in the fume hood. Collaboration between academia and industry opens access to high-throughput screening, shortening the feedback loop between idea and data. Supply chain transparency matters here: sourcing high-purity precursors, documenting batch history, and closing information gaps with customers. That’s how innovation turns safe and sustainable.
Toxicologists work methodically, step by step, before labeling chemicals as benign or hazardous. Halogenated aromatic ketones follow an uncertain path, as lab data and environmental experience sometimes diverge. Some studies have shown DNA-binding potential or effects on metabolic enzymes, though conclusive in vivo data can lag behind in vitro warnings. Repeat-exposure animal studies track organ weights, blood chemistry, and excretion patterns, while analytical teams check for persistent residues in soils or wastewater. Regulatory committees demand rigorous validation, especially if the compound drifts toward broader market use. For now, safety datasheets recommend controlling dust and vapor, and limiting exposure, not out of theory but because real-world toxicity cases often come back to unreported spills and unforeseen reactivity. Ongoing research closes these gaps, shaping regulations and company policy.
Demand for designer chemical building blocks shows no signs of slowing, especially among emerging fields such as advanced materials, green solvents, and precision pharmaceuticals. With ongoing pressure from customers and regulators, companies race to develop even safer, more sustainable analogues, and to perfect existing synthesis and handling procedures. Digitalization in chemical R&D will only magnify these efforts, linking research findings to global markets with unprecedented speed. As society’s needs shift toward reduced environmental footprint and greater product accountability, researchers engaged in this field will find that every new insight and incremental improvement opens new tracks for both commercial and scientific breakthroughs. The future of 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone, and related molecules, will keep evolving as chemists, engineers, and policymakers tackle the tensions between performance, safety, and sustainability.
Let’s talk about a structure that chemists, and even non-chemists, find interesting once you dig beneath the surface: 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone. The name might be a mouthful, but each part says something important about how the molecule is built. It features two connected benzene rings—a setup familiar in pharmaceuticals and specialty materials. Across these rings, chemists have placed a bromine, a chlorine, and an ethoxy group. Toss a ketone group in there, and you get a unique compound with a handful of tricks up its sleeve.
The molecular backbone starts as benzophenone: two benzene rings linked by a carbonyl (C=O group). The "5-Bromo" and "2-Chloro" mean those spots on one ring carry a bromine and a chlorine atom, both heavier-than-average elements you don’t see stuck on just anything. The "4'-Ethoxy" points to an ethoxy group—a two-carbon chain capped by oxygen—attached at the 4-position of the other benzene ring. For chemists, the full name acts almost like a set of building instructions.
Halogens such as bromine and chlorine change more than just the weight of a molecule. They influence how it interacts with other chemicals, how it dissolves, and, in many settings, how it targets biological systems. Drug designers look at halogenated compounds because these atoms boost something called lipophilicity—how well a molecule blends into fats. This adjusts how the body absorbs and stores potential medicines. Ethoxy groups offer a different leverage. By increasing solubility and shifting electronic properties, ethoxy substitutions can help chemists tweak the activity or stability of the molecule.
Through these chemical attachments, 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone gains new characteristics. It doesn’t just rest as an academic curiosity. It bridges lab curiosity with practical application, especially in chemical research focused on custom building blocks for more complex targets.
Molecules like this show up in screens for new drugs, in dye research, and occasionally as part of specialty polymers. Academic papers reference close relatives in journeys to develop anti-inflammatory or anti-cancer agents, sometimes because halogens nestle into enzyme pockets that less heavy groups can’t touch. Printouts from mass spectrometers around the globe have identified derivatives of similar compounds in ongoing pharmaceutical projects. That’s not speculation—PubChem and Reaxys databases track real hits for these frameworks in medicinal chemistry pipelines.
Making 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone in the lab takes clever planning. The different groups around the rings cannot simply be slapped on in any order. Chemists learn through trial and error that adding bromine reacts best at a certain stage. Putting on the ethoxy group later lets them sidestep unwanted side reactions. I’ve stood at the bench, watching others tinker with the order of those substitutions—changing one step can shift the whole outcome. Every extra group can slow down or block further reactions, so process chemistry relies on real-world experience instead of trusting theory alone.
Anyone aiming to design related molecules quickly runs into availability and safety concerns. Not all halogenating agents are easy or safe to handle, especially outside a controlled setup. Green chemistry pushes for less toxic reagents and smarter methods. Flow chemistry—moving chemicals past each other in tubes instead of mixing everything in big pots—helps manage risks. Automated synthesis and AI-assisted planning can narrow down better, safer ways to reach complicated molecules like this one.
The structure of 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone tells a story about precision, chemical intuition, and the evolving toolkit of organic chemistry. Tracking its impact in both research and manufacturing shines a light on the intersection of scientific curiosity and the ongoing push for new solutions.
Anyone who’s spent real time in a chemistry lab knows certain molecules hold far more value than their mouthful of a name might suggest. 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone happens to be one of those. Rather than sit on a dusty shelf, this compound winds up at the center of some creative, hands-on research. For context, it’s a building block in the world of organic synthesis—a stepping stone as researchers across the globe chase new pharmaceuticals and specialty chemicals.
Pharmaceutical breakthroughs rarely rely on simple, single-step processes. Chemists use molecules like this one to build complexity—layer by layer—until a drug candidate emerges. 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone fits into medicinal chemistry as a core intermediate. Its shape and reactive sites help scientists tweak molecules, either to block biological targets or fine-tune how a drug behaves in the body. The halogen atoms (bromo and chloro) open up routes for more chemical tinkering; the ethoxy group changes the way the molecule dissolves and interacts, making it a favorite in projects looking to boost drug delivery or stability.
Sometimes, time in the lab feels like a long slog, especially with how often teams chase new lead molecules for conditions like cancer, epilepsy, or rare autoimmune disorders. All that effort requires chemical tools able to withstand a range of experimental conditions. I’ve watched colleagues run reactions that push temperature or pressure, searching for the right yield. This compound stands up to such challenges, letting labs crank out dozens of derivatives, then screen them for promising biological activity.
Pharmaceutical research isn’t the only arena where this molecule matters. Some specialty chemicals, used in advanced materials and dyes, start with intermediates like 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone. Researchers developing organic electronics—think small, bendable devices or smart sensors—sometimes use similar building blocks while exploring new polymers or semiconductors. These kinds of compounds come into play when aiming for specific optical or electrical properties, since tiny tweaks in structure can yield big swings in performance.
Over the years, I’ve seen student teams try to design light-stable materials for anti-counterfeiting features or medical imaging. The chemistry behind those features draws directly from scaffolds similar to this one. A working knowledge of how to swap out groups, or how the compound behaves under harsh light or high temperatures, helps push the whole field forward.
Widespread use brings some responsibility, though. These halogenated compounds can linger in the environment if users finish a reaction, discard waste, and don’t follow proven disposal protocols. Realistically, not every university or small firm has easy access to advanced destruction options, so more research into green chemistry routes for synthesis and breakdown of such molecules makes sense. Partnerships with waste management firms, and strong oversight by regulators, help shrink the footprint of even small-scale labs. Still, cutting-edge chemistry shouldn’t come at the cost of long-term health or soil quality, so continued investment in cleaner processes stands as a priority.
In my own experience, I’ve watched regulations move from checkbox compliance to real collaboration between chemists and environmental scientists. Sharing best practices—down to the nitty-gritty of solvent selection and waste tracking—pays dividends in the end.
The story of 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone is still being written in countless labs. As drug pipelines change, as electronics get smarter and smaller, molecules like this stay relevant—if we use them wisely and responsibly.
Many chemicals in laboratories and industry don’t grab much attention until something goes wrong. 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone isn’t a household name, but it fits right into this category. Experience in research settings shows that mishandling chemicals, even ones that seem stable, can spoil months of hard work or compromise safety. Problems usually start small — a little moisture sneaks in, temperature gets ignored over the weekend, or someone overlooks sealing a bottle. After working with similar diphenylmethanone compounds for a decade, I’ve seen first-hand that leniency with storage usually ends with degraded samples or, worse, health risks for lab staff.
Looking at 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone specifically, its stability comes into question under fluctuating environmental conditions. Although the molecule isn’t extraordinarily sensitive, it absorbs moisture from the air and breaks down faster in warm or well-lit rooms. Every reputable supplier recommends keeping it in a tightly closed container in a cool, dry, and dark area—typically inside a chemical refrigerator or a desiccator. High humidity speeds up hydrolysis, and elevated temperatures accelerate decomposition, risking a loss of activity for anyone relying on its reactivity in synthetic pathways.
In research environments where a reagent like this costs hundreds of dollars, losing a batch only because the container sat near a sunny window makes no sense. The yellowing of the powder or a strange odor from the vial are early signs of breakdown, often followed by inconsistent results in experiments.
Placing the vial inside a screw-top amber bottle limits light exposure. Tossing in a few silica gel packets absorbs stray moisture. Store the bottle on a refrigerator shelf reserved for chemicals, away from food and other volatile substances. Every label should carry the date of receipt and the last date opened to avoid the trap of using something well past its prime. These hands-on details prove their worth during audits and, more importantly, when an experiment behaves just as predicted.
In my lab days, an incident sticks with me: a colleague grabbed what looked like a fine sample of another diphenylmethanone stored at room temperature in a clear bottle. Weeks later, our project hit a wall until retesting revealed a cocktail of impurities. It cost the team both time and credibility. That setback changed our handling routines overnight. Investing a bit of effort upfront in controlled storage minimized headaches. In fact, chemical stability data from suppliers back this up—a temperature drop from 25°C to 4°C routinely doubles shelf life for aromatic ketones.
These days, lab management tools with RFID tracking and audit trails make it easier to keep tabs on storage. Outdated, anonymous vials get spotted quickly, reducing risks to both experiments and people. Manufacturer guidelines exist for a reason; following them builds a culture of discipline and quality. With growing research costs and scrutiny, attention to small details—like how to store 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone—just makes sense.
Walking into a lab, most people set their trust on the safety data sheets stapled to shelves. I’ve seen the chemical hazard charts and, truth be told, many compounds with long, complicated names get glossed over. Still, names like 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone deserve more than a background role. This one flags more than curiosity—handling this compound isn’t just business as usual.
This molecule, built from halogenated benzophenone, holds a track record for health and environmental questions. Halogens like bromine and chlorine give chemical stability and reactivity, but they also mean the compounds slip into cells and disrupt normal functions. I remember a study out of Europe pointing at bioaccumulation with similar halogenated substances—bodies struggle to break them down. Once in, they stick around.
Eyes, skin, and lungs take the brunt of exposure. Benzophenone derivatives often irritate, and some spark allergic reactions. Skin rashes or eye reddening show up before anybody thinks about more serious long-term impacts. Chronic exposure to halogenated chemicals sometimes raises questions about the risk of organ damage or hormone disruption. Regulatory agencies in the U.S. and EU haven’t flagged this exact compound as a top-tier hazard, but they lean cautious with its relatives.
Anyone working with 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone can’t rely on luck or basic ventilation. Gloves, goggles, and coats form the first line. Nobody grabs this stuff barehanded. Proper fume hoods mean a lot—a small spill on the bench without airflow may lead to bigger problems than a ruined experiment. Spills of halogenated organics just don’t wipe up with a paper towel. They linger, they stain, and the smell alone grabs your throat.
Disposal rarely gets the attention it needs, and that’s a shame. Sending waste straight down the drain causes headaches later. I’ve watched wastewater folks run extra tests whenever a lab near groundwater dumps organics. People think environmental rules pile on too many restrictions, but I’ve also seen rivers take years to recover when chemicals slip past.
Many chemists handle dozens of intermediates every week. They tell themselves that small-scale chemistry doesn’t add up to much. History proves otherwise. In the 1970s, nobody looked sideways at dumping halogenated compounds until whole populations of fish turned belly-up. The smaller the molecule, the easier it migrates—through a glove, up the nose, or down the drain.
The risk stays manageable only with routine attention. Regular training pays off more than laminated hazard sheets taped on walls. PPE supply has to be steady. Clean benches and daily equipment checks keep rogue chemicals from escaping. People need to read the latest data, review their own habits, and ask hard questions about process changes. This compound is just another in a long line of chemicals that calls for respect.
Industry and academia still wrestle with balancing safety and research goals. One fix centers on green chemistry—designing ways to build molecules like this one but skipping the most toxic starting materials. Researchers with deep experience offer simple advice: treat every halogenated compound as a health risk. Swap out or scale down where possible. Secure storage prevents “mystery spills” and labels that fade too soon.
Sharing close calls and mistakes in group meetings—no matter how embarrassing—often improves habits faster than any email memo. Safety logs give clues to weak routines or outdated practices. Every bottle of 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone reminds me of the choices between rushing through lab work or hitting pause for safety.
Most people working in chemical labs can recall at least one moment involving a botched experiment caused by hidden impurities. With chemicals like 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone, purity quickly becomes the backbone of trustworthy results. Suppliers usually list purity as a percentage, often starting at 97% and going up to 99% or higher. These numbers aren’t just marketing speak; every extra point above 97% means a smaller risk of unexpected side reactions, unpredictable toxicity, or batch-to-batch inconsistencies. R&D teams count on high-purity reagents so they can trace outcomes to their own methods rather than having to dodge ghost contaminants.
Some end users, especially those scaling from bench chemistry to pilot processes, won’t settle for less than 99% purity, and for good reason. Unwanted isomers or trace halides lurking in the remaining percentage can bring headaches to both process and analytical chemists. Purity reports—including NMR, HPLC, and elemental analyses—are not optional extras; they’re the safety net that keeps things above board once the work starts ramping up. Whenever I’ve checked certificates of analysis, I look for these numbers, not just a basic label that says “assay: 98%.”
Reliable suppliers typically report assay values for 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone in the range of 97-99%. Sometimes an HPLC trace will accompany this, giving a quick look at how clean the material truly is. Documentation usually breaks down the assay, moisture content, and residual solvents. From my own experience sourcing such chemicals, I value suppliers who are upfront about possible byproducts. If a certificate feels vague or missing details, it’s often a warning sign.
Having a compound at 98%+ purity can speed up risk assessments for labs focused on drug discovery or toxicology testing. Impurities can introduce unknown factors, particularly in biological assays. Regulatory compliance checks—including those for companies following ISO or cGMP standards—closely examine these purity levels. In one project I joined, we faced delays because a shipment only met 95% purity, nudging us into extra rounds of quality controls. That minor 3% gap mattered to our results and our bottom line.
Straightforward steps can help ensure the chemical purchased meets the needed specification. Asking questions before purchase—such as requesting a recent certificate of analysis or checking for batch-specific documentation—brings clarity. If there’s uncertainty in reported values, bringing samples in for third-party verification helps mitigate risk. Staying in regular contact with suppliers and building a history of trust also lowers the frequency of surprises.
The spread between 97% and 99% purity for 5-Bromo-2-Chloro-4'-Ethoxydiphenylmethanone isn’t just academic—it’s the difference between chasing down artifact data and working with a chemical foundation that researchers can trust. Those extra few points of purity represent less time spent troubleshooting and more time building results that stand up under scrutiny.
| Names | |
| Other names |
NSC401865 AKOS015889470 SCHEMBL14174529 |
| Pronunciation | /faɪv-ˈbroʊmoʊ-tuː-ˈklɔːroʊ-fɔːrθ ˈiːθɒkˌsi-ˌdaɪˈfenəlˈmɛθəˌnoʊn/ |
| Identifiers | |
| CAS Number | 885273-44-1 |
| Beilstein Reference | **3289276** |
| ChEBI | CHEBI:87636 |
| ChEMBL | CHEMBL1386703 |
| ChemSpider | 28637998 |
| DrugBank | DB08357 |
| ECHA InfoCard | 03-212-1406113243-94-0000 |
| Gmelin Reference | Gm 24 627 |
| KEGG | C18960 |
| MeSH | D017356 |
| PubChem CID | 136885277 |
| RTECS number | HP0511000 |
| UNII | QX97P7AE3S |
| UN number | UN2811 |
| CompTox Dashboard (EPA) | DTXSID5062587 |
| Properties | |
| Chemical formula | C15H12BrClO2 |
| Molar mass | 335.68 |
| Appearance | White to Off-White Solid |
| Odor | Odorless |
| Density | 1.43 g/cm³ |
| Solubility in water | Insoluble |
| log P | 3.9 |
| Vapor pressure | 0.0000227 mmHg at 25°C |
| Acidity (pKa) | Acidity (pKa): 15.6 |
| Basicity (pKb) | pKb = 11.91 |
| Magnetic susceptibility (χ) | -79.41×10⁻⁶ cm³/mol |
| Refractive index (nD) | 1.591 |
| Viscosity | Viscosity: 1.09 cP (Predicted) |
| Dipole moment | 3.5615 Debye |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 385.3 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -119.2 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -7236.7 kJ/mol |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes skin irritation. Causes serious eye irritation. May cause respiratory irritation. |
| GHS labelling | GHS07, GHS08 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H315, H319, H335 |
| Precautionary statements | Precautionary statements: P261, P264, P271, P272, P273, P280, P302+P352, P305+P351+P338, P321, P332+P313, P333+P313, P337+P313, P362+P364, P501 |
| NFPA 704 (fire diamond) | Health: 2, Flammability: 1, Instability: 0, Special: |
| Flash point | 156.6 °C |
| Lethal dose or concentration | LD50 (oral, rat): >2000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Rat oral >2000 mg/kg |
| NIOSH | BR2080000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 10 mg |
