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Chemical discovery rarely follows a straight path, and 3-Chloro-1,2-propane-1,1,2,3,3-pentaol stands as a clear example of this journey. This compound's story begins in late-20th-century synthetic chemistry labs, where scientists kept looking for new chlorinated, polyhydroxy intermediates to build a bridge between simple feedstocks and more functional specialty molecules. Curiosity about glycerol modifications, inspired by demand for more specialized reagents in resin research and the surfactant industry, led to systematic lab work. Researchers experimented with a strong curiosity, combining propanediol and glycerol analogs with various halogenation techniques. As methods for selective chlorination grew more accessible, the rise of compact instrumentation sped up identification and characterization. A compound as unique as 3-Chloro-1,2-propane-1,1,2,3,3-pentaol rarely came to light unless persistent tinkerers paid close attention to reaction side streams, lab notebook scribbles, and those odd batches that did not look quite like the target but still intrigued the chemists. A blend of academic curiosity and commercial application made this material a subject for further probing, not only in Europe and the US, but also across labs in Asia where novel polyols caught plenty of attention. Chemists pushing to overcome bottlenecks in coatings, drug synthesis, and high-value polymer production often recognized this “pentaol” as a potential problem-solver, long before it showed up in formal supply catalogs or safety guidelines.
One glance at the structure says a lot about what makes 3-Chloro-1,2-propane-1,1,2,3,3-pentaol so unique. The chemical carries a single chlorine atom attached to a three-carbon skeleton heavy with hydroxyl groups—five in all. This combination sets up a playground for organic transformations. Its crowded backbone and the presence of both electrophilic and nucleophilic centers give the pentaol a quirky character. People working with this compound often find themselves facing unexpected viscosity, surprising solubility patterns, and quirky reactivity in both aqueous and non-aqueous environments. Because of these properties, this molecule earned a reputation for opening new doors for reaction design but also causing a few headaches along the way. The world of specialty chemicals moves fast, and materials like this don’t last long on the sidelines; once its synthetic potential comes into focus, chemists keep it at hand for building new reagents and introducing unconventional motifs into larger molecules.
In practice, this compound tends to present as a viscous syrup or a sticky crystalline solid, depending on temperature and the presence of other solvents. Five hydroxyl groups make for a heavily hydrogen-bonded network; you will spot it soaking up ambient moisture in a humid lab and clinging to glassware. The chlorine atom does more than add weight; it shakes up the reactivity, making the molecule respond differently to bases and nucleophiles than similar polyols like glycerol. Reasonably soluble in water and polar organic solvents, the pentaol brings excellent miscibility with alcohols and glycols but only limited solubility with classical nonpolar organics. Its boiling and melting points remain less commonly charted in literature, no surprise given the sticky, hydrophilic character, but chemists often circumvent issues by prepping solutions right before use. Handling such a compound on the bench lets you see the trade-offs of highly functionalized molecules: constant attention to purity, monitoring for byproduct formation, and dealing with challenges in isolation and drying.
As with many specialized reagents, standardization takes time and tends to follow demand. Early batches from research-grade suppliers rarely came with elaborate technical certificates or detailed chromatograms. Quality hinged most on the right signals in NMR, spot tests for residual chlorides, and sharp, reproducible peaks in thin-layer chromatography. Today, reputable labs characterize each batch with high-resolution NMR, FTIR, and mass spectrometry. Labels may carry the classic chemical name, a CAS number if registered, and gross purity; less frequently, you may see the full set of hydroxy numbers or specifications for residual solvents and moisture. For practical chemists, what's most important is trust in the supplier’s analytical methods and assurance that no reactive contaminants slipped through during workup or storage. The presence of multiple chiral centers can pose real-world challenges in characterizing stereochemistry, and few users will expect or need enantiomerically pure product unless further resolution follows downstream.
Synthesizing 3-Chloro-1,2-propane-1,1,2,3,3-pentaol calls for careful handling and patient incremental work. Chemists often start from accessible triols like glycerol, introducing chlorine using routes with thionyl chloride, phosphorus oxychloride, or milder bases when available. Protecting group strategies provide the flexibility required to block certain alcohol functions, expose target carbons for halogenation, and then walk these groups back to the original pentaol. Another path includes ring-opening of epichlorohydrin followed by selective hydroxylation. None of these reactions proceed at lightning speed, as complex mixtures and over-chlorinated byproducts demand careful TLC monitoring and frequent purification cycles. A well-tuned procedure balances cost, safety, and scalability, always wary of the environmental footprint left behind by halogenated waste and aqueous washes. On paper, the chemistry looks straightforward; in practice, a skilled chemist’s patience and a reliable fume hood make the difference between success and frustration.
The multi-hydroxyl character of this compound offers room for creative exploration. Once the compound is in hand, chemists have a field day with esterifications, etherifications, selective oxidations, and even efforts to swap out the halogen. Its propensity for both intra- and intermolecular hydrogen bonding shapes reactivity in ways that sometimes defy prediction. Chlorine at the terminal carbon gives a handle for substitution chemistry, with classic nucleophiles like amines and thiols generating a slew of secondary products. Each hydroxyl can act as a launching pad for designer transformations, delivering acyl, alkyl, or even polymerizable motifs. Work in polyurethane chemistry illustrates the advantage of plugging in a pentaol for extra crosslinking, and surfactant researchers look at the backbone as an avenue for tuning solubility and interface behavior. On the downside, unwanted reactions—self-condensations, slow hydrolysis in damp storage, or even minor decomposition under high heat—can complicate scale-up and storage. That unpredictability is what draws talented reaction designers: this pentaol challenges people to tailor techniques rather than follow a script.
If you talk to a chemist in another country or browse international catalogs, creative synonyms crop up. Common names include “chloropentahydroxypropane” or “chlorinated glycerol pentaol,” giving a nod to both the structure and the parent compounds. Several catalogs record alternate designations based on ring-opened chlorohydrin or pentaol models. Lab groups give it shorthand like “Cl-pentaol” on bench-side labels, sometimes followed by a project code if multiple variants have been tried. The lack of a long marketing track record means fewer regional or trade names compared with established glycols. Synonyms help bridge language barriers but can also lead to confusion over details—whether it’s the same substitution pattern or only a closely related analog. As research advances, consistent naming conventions and reliable CAS numbers prevent mix-ups, especially for those cataloging results for publication or seeking regulatory clarity.
Dealing with chlorinated, highly functionalized small molecules calls for strict lab safety. Years of bench work show that accidents most often follow routine handling: incorrect ventilation, splashes from sticky liquids, or casual disregard for proper PPE. Reviews of related halogenated compounds underscore the risk of skin and respiratory sensitization, even if each new analog brings different risks. Best practices include double gloving, a sturdy lab coat, and working inside a well-ventilated hood. Few researchers like leaving a sticky pentaol on a shared workspace, as it attracts dust and soaks up water, further complicating clean-up. Storage in dark, cool conditions reduces slow decomposition and limits accidental contact with incompatible reagents like strong bases or oxidizers. As regulatory agencies step up surveillance of halogenated compound handling, up-to-date MSDS consultation and clear lab training show their value on a weekly basis. The trade-off for powerful, reactive molecules is a step-up in mindfulness and support from well-prepped facilities.
Ask a handful of industrial and academic chemists where this molecule finds use, and you'll hear a healthy mix of ideas. Some see it adding value in crosslinked polymer matrices, seeking the unique blend of flexibility, adhesion, and solubility that a pentaol can lend to coatings. Others experiment with its backbone in surfactant research, banking on oddball hydrophile–lipophile balance tuning for specialty cleaning, dispersants, or emulsifiers. Its reactive side creates routes to novel drug precursors, linking to chiral auxiliaries or complex intermediates typically off-limits to simpler glycols. On a smaller scale, synthetic biochemistry groups examine the potential for enzyme-driven modification, hoping to harness selectivity absent in harsh organic conditions. Materials science teams weigh its role in modifying membrane properties or introducing crosslink points in hydrogels built for controlled release or sensor applications. What binds these efforts is the search for new performance benchmarks—better physical properties, more tractable reactions, or value-added features over existing triols and tetrols.
Research on chlorinated polyols, and this one in particular, brings together motivated teams from both academia and industry. Frequent citations in patent filings and specialty journals tell the story of ongoing effort. The last decade saw a growth in computational design and real-world testing of derivatives, as scientists push for better catalysts, less waste, and greener routes. As environmental regulations shift, a big driver now revolves around cleaner synthetic methods, like using water as a solvent or replacing hazardous chlorination reagents with safer options. Academic groups keeping an eye on structure–activity relationships continue to map out the molecule’s influence in complex chemical environments. Those working in application development value quick feedback loops, feeding results from bench tests right into prototype coatings, adhesives, or specialty surfactants and reporting back with insights about performance (or unexpected problems). Collaborative relationships between suppliers, academic labs, and end-users keep research moving faster and steadier, especially as niche markets ask for more reliable materials and less environmental baggage.
Assessing toxicity takes more than a quick scan of related compounds. While plenty is known about other polyols and chlorinated small molecules, each tweak to the structure can result in different hazards or breakdown pathways. Initial studies on this pentaol indicate that the chlorine group introduces mild irritant behavior, especially for skin and mucous membranes. Animal and cell-line work flagged possible cytotoxic effects at high dosages, which comes as no surprise for compounds bearing both halogen and multiple hydroxy functions. Chronic exposure studies still lag behind, in part because industrial throughput is lower than big commodity chemicals. Researchers call for broader tests that dig into metabolic byproducts, risks of environmental persistence, and potential endocrine or developmental impacts. Workers in the field already understand the value of rigorous handling, routine health monitoring, and swift response to odd lab symptoms (like headaches or unexpected skin rashes.) As wider adoption looms, lessons from other chlorinated intermediates—like trichloropropane or similar legacy solvents—echo in regulatory guidance and the push for more sustainable alternatives.
Looking forward, this compound’s fate sits at the intersection of discovery and responsibility. Smart chemical engineering offers a route to less toxic, more biodegradable analogs, provided the industry steps up to share data and insights. The appetite for polyfunctional materials is on the rise, as everything from battery research to sensor design seeks molecules that bring more than one trick to the table. If further toxicity data clears the way for safer use, expect a surge in downstream applications, particularly where crosslinking and fine-tuned polarity make a competitive difference. Greener synthetic methods, like catalytic hydroxylation or enzymatic modification, present another leap, reducing waste and cost. Early-career chemists and established process engineers get a chance to sharpen their skillsets tackling materials just like this one: not pure commodity, yet not so exotic that industrial scale seems impossible. Advocacy for safer practices, transparency in research findings, and tighter links between technical teams will all carry big weight in shaping this material’s legacy—long after the raw technical descriptors fade from memory.
Stepping into the world of specialty chemicals often feels a lot like walking through a maze. Each compound, with its own long name and longer list of peculiar properties, has a purpose. 3-Chloro-1,2-propane-1,1,2,3,3-pentaol isn’t a household name. That’s a signal. It rarely pops up outside of chemical plants or technical journals. Still, its structure—loaded with both chlorine and multiple hydroxyl groups—tips the hand of its real-world value.
Many industries look for compounds that act as middlemen in bigger syntheses. I spent time in a mid-sized chemical plant—places like that don’t want exotic for the sake of exotic. They want reliable results, fewer safety headaches, and affordable price tags. 3-Chloro-1,2-propane-1,1,2,3,3-pentaol has a quirky design: one chlorine atom surrounded by five hydroxyl groups. That means strong reactivity, which usually translates to roles in making other molecules. Chemists call these kinds of compounds “intermediates.”
Plastic manufacturers have a soft spot for small, versatile molecules—they’re often in the market for additives that tweak the flexibility and toughness of polymers. Traces of this compound might find their way into formulations for specialty plastics, hydrogels, or even tough resins. A structure loaded with those -OH groups is built for connecting with other chemicals. Cross-linking comes easy. That’s how the plastics industry tunes materials to stand up to stress, heat, or humidity.
During a side project in a pharmaceutical lab, I learned that almost any compound with both chlorine and hydroxyl groups gets attention from drug designers. The skeleton of 3-Chloro-1,2-propane-1,1,2,3,3-pentaol can morph under the right conditions, picking up modifications until it forms the backbone of a new medicine or diagnostic agent. Medicinal chemists sometimes chase unusual structures because they can offer unique ways to attach “functional groups”—the business end of pharmaceuticals. A rigid but reactive molecule like this fits the bill, delivering new options for carbon or nitrogen attachments. That opens doors for research into active ingredients and molecular probes.
Outside the pharmacy, there’s a real market for compounds with big polar character. Cleaning products, for example, perform better with agents that can dissolve both greasy and mineral-based dirt. Molecules with multiple hydroxyl groups shine in this role. Some chemical catalogs even list derivatives of this compound as potential surfactants or chemical dispersants. In coatings, surface chemistry is everything. The right additives help paints grip metal, glass, or plastics, adding value and durability to everything from car bodies to power tools.
It might sound technical, but ignoring the risks of chlorine-containing compounds is a quick route to disaster. I’ve seen small mishaps cause big headaches. Chlorine brings reactivity, but that can lead to environmental or health issues if disposal isn’t tight. Regulatory agencies—EPA in the United States, ECHA in Europe—zero in on chemical releases, pushing companies to tighten up their waste streams and develop safer substitutes. Proper protocols and modern waste-treating tech solve many issues, but vigilance remains the best guardrail.
The search never stops for cleaner, safer alternatives. Researchers dig into plant-based building blocks and recycled feedstocks. At the same time, companies rethink synthesis routes, switch to greener catalysts, or even adopt closed-loop manufacturing where every scrap finds a second life. It’s not only about compliance. It’s about matching innovation with responsibility—an approach more young chemists refuse to compromise.
3-Chloro-1,2-propane-1,1,2,3,3-pentaol—just reading that mouthful makes me picture racks of containers, each needing careful handling. In the lab, you develop respect for molecules that mix reactivity with toxicity. Organic chemicals with chlorine—or multiple alcohol groups—demand the same respect you’d give a swinging blade. Skin contact, vapors, splashes in the eye: a casual mistake becomes a real problem fast.
Chlorinated alcohols act as irritants, and repeated skin exposure sometimes leads to rashes or burns. Eyes don’t forgive splashes of reactive organics, either; even small droplets will burn. The risk compounds when these substances are volatile or produce fumes. It’s tempting to think, “I’ll just be quick,” but I’ve watched hasty coworkers reach for a wash station with real panic. A few minutes could spell a trip to urgent care.
A strong set of safety habits saves you trouble. I grab gloves—nitrile, not just latex, since those tend to hold up to solvents. Goggles every single time. No safety glasses, not when even a tiny droplet could end up in your eye. Lab coats protect arms and clothes. Working in a fume hood also shields your lungs. Underestimating the vapor risk leaves you one breath away from a bad headache or, worse, a chemical injury to the airways.
A shelf lined with glass bottles can turn to chaos if one leaks or breaks. This chemical’s structure signals a potential for slow decomposition or interaction with air, so I always ask about expiry and storage temperature. Sealed containers, dry and cool shelves, away from sunlight—simple steps, but I’ve seen accidents start with a cracked lid on a hot day.
Don’t pipette by mouth, don’t walk away mid-transfer—these rules are drilled into every chemist, but you only need one slip. Clean up spills right away with absorbent pads designed for organic solvents; water may just spread it or cause exothermic messes. I always check that spill kits are up to date. The best labs post material safety data sheets on the wall where everyone can see them. Knowing where the eyewash and showers sit means you don’t lose precious seconds if a spill goes wrong.
Proper chemical disposal means collecting waste in compatible bottles, clearly labeled, and never mixing with acids or oxidizers. I once caught a colleague ready to dump an organic waste into the wrong drum, and catching the error spared the whole team a fire risk. Regulations keep changing, so I keep a folder open with local laws on chemical disposal right on my desk.
Working with chemicals like 3-Chloro-1,2-propane-1,1,2,3,3-pentaol means treating each step like it matters. Protective gear, dedicated disposal, strict attention during transfers—these aren’t just bureaucracy. They help you finish a lab session with clean skin, clear lungs, and an intact career. If you ever doubt whether you’re being cautious enough, remember: you only get one pair of hands, one set of lungs, and one set of eyes.
I always encourage training refreshers and clear signage. Shortcuts only satisfy in the moment, while accountability and knowledge build a safer lab culture that keeps everyone working—not recovering at the doctor’s office. Safety isn’t just for rule-followers; it protects everyone, including the rookie who just put on a lab coat for the first time.
Chemistry shapes so much of how we interact with the world. I remember being fascinated the first time I tried to draw out a complex organic compound, and 3-Chloro-1,2-propane-1,1,2,3,3-pentaol would have tripped me up for sure. Just looking at the name, there’s a lot happening: a propane backbone, a chloro group, and five hydroxyl groups squeezed onto three carbons. Structurally, the backbone follows propane’s three carbons in a row. The "3-chloro" tells me a chlorine atom attaches to the third carbon. Every time I see “pentaol,” I know there are five alcohol (–OH) groups in the mix. What jumps out here is just how packed this molecule is, especially since the locants—1,1,2,3,3—mean carbon 1 and 3 each carry two hydroxyl groups, and carbon 2 brings in one of its own.
If I sketch it out, I see something like this: starting at the first carbon, two –OH groups latch on. The second carbon ties to one –OH. The third carbon has a chlorine and, again, two –OH groups. It’s almost crowded at the atomic level, and those extra hydroxyls really affect what this molecule can do.
This structural arrangement transforms the chemical’s behavior. More hydroxyl groups mean more hydrogen bonding. That translates to high solubility in water and strong interaction with polar solvents. The chlorine atom introduces another dimension. Chlorinated chemicals have a history of being both useful and risky: think about chlorinated solvents or disinfectants. In compounds like this one, chlorine’s presence can alter reactivity or toxicity. Safety-wise, my experience reminds me always to respect these halogenated compounds. They can pop up with unexpected consequences on human health or in the environment.
On an industrial or research level, those multiple –OH groups lead to possibilities. Pentaols aren’t common in pharmaceuticals or agrochemicals, but their strong polarity makes them useful as intermediates—essentially stepping stones—toward other specialized chemicals. I’ve seen polyols used to build up certain types of polymers or to tweak reactivity in drug discovery. I’d wager this molecule could be investigated for similar roles, though the crowded structure raises stability questions that researchers must test in the lab.
Chemicals loaded with functional groups often raise flags in safety and waste management. I’ve seen more than one research team caught off guard by the hazards of chlorinated alcohols: they’re not always easy to dispose of safely, and sometimes they resist breaking down in nature. This can create headaches for both labs and larger facilities. Regulatory bodies keep a close eye on such structures, and any widespread use brings the need for solid handling protocols. Wear gloves, use a hood, and treat every new chemical as a potential unknown until proven otherwise.
Researchers win by building out clear safety data for new chemicals. It’s not enough to synthesize and characterize; teams need to study how it degrades, what products come from burning or aging, and whether it persists or breaks down in water streams. This approach doesn’t just protect workers—it keeps chemicals with long-term risks from creeping into the environment. I’ve found that spending time on this early in development saves a lot of trouble downstream. That’s common sense built from years of lab experience, and it always pays off when new chemicals like 3-Chloro-1,2-propane-1,1,2,3,3-pentaol start to see wider interest.
A lot of people think handling chemicals means white coats and secure labs. Sometimes, folks underestimate the actual risks sitting on the shelf in a plain bottle. 3-Chloro-1,2-propane-1,1,2,3,3-pentaol doesn’t sound as alarming as something like “hydrofluoric acid,” but that calm can trick you. Even chemicals with less notoriety can lead to skin irritation, respiratory trouble, or, occasionally, worse effects if not treated with respect.
Every bottle of this compound deserves its own designated spot. Chemical compatibility charts do not just exist for show; mixing chlorine-containing substances with the wrong chemical neighbor often means headaches, at best, and nasty reactions, at worst. This compound should not find itself near strong acids, oxidizers, or reducing agents. Fumes that result from chemical mishaps have sent seasoned researchers home for the week. I once saw a seemingly minor storage oversight ruin an entire batch of samples in an academic lab, forcing a costly clean-up. It’s the little things that throw off weeks of careful work.
Keep 3-Chloro-1,2-propane-1,1,2,3,3-pentaol in a tightly closed container. Moisture sneaking in can change the composition or, worse, start a slow decomposition. The best spot is a cool, dry, well-ventilated area. Direct sunlight raises both the container’s temperature and the risk of breakdown. Most reputable chemical suppliers use amber glass containers for a reason — they protect contents from UV rays that trigger unwanted reactions, so it’s wise to do the same.
Labeling matters, too. A sharp label with the full chemical name, date received, and hazard information provides an instant reminder. Nurses and lab techs wouldn’t dare trust a half-peeled sticky note, and neither should you. If the bottle’s seen better days, switching it out helps avoid leaks or breakage from degraded plastic or glass.
I used to run a shared university stockroom. More than once, someone left bottles close to heat sources, like radiators or windows, only to discover warped labels and caked-on residue the next week. The simple act of moving volatile chemicals to a lower, temperature-stable shelf kept accidents at bay. A friend’s start-up chemistry lab once lost thousands to a preventable spill; their oversight was not isolating incompatible chemicals. Incidents felt even worse because the warning signs existed all along.
Storing this compound apart from food, drinks, and personal items makes sense for health and safety. Take regular inventory of chemical stocks, and check expiry dates; chemicals don’t age gently. Make sure only trained personnel access the storage area, and always offer gloves and goggles, not just a stern safety speech. Spill kits, eyewash stations, and clear instructions on the wall provide backup. If small labs or workspaces seem cramped, wall-mounted cabinets with solid lock systems help maximize limited real estate.
Proper storage doesn’t have to feel like an overwhelming science project. Treating 3-Chloro-1,2-propane-1,1,2,3,3-pentaol with a steady routine of clear labeling, isolated placement, and temperature control protects both the folks working around it and the investment behind every bottle. Accidents rarely strike without warning; they usually walk through open doors left by small lapses in daily care.
Looking at a tongue-twister like 3-Chloro-1,2-propane-1,1,2,3,3-pentaol makes chemistry feel like decoding a secret message. As someone who learned the ropes of chemistry in college labs, it’s easy to recognize the clues about how a molecule will behave with water by just glancing at its structure. This compound’s name reveals five hydroxyl (-OH) groups and a single chlorine. Hydroxyl groups share a reputation for grabbing water molecules, thanks to their strong tendency to form hydrogen bonds.
Most people chalk up water solubility to “just mix it in and see,” but let’s dig a bit deeper. Every -OH group increases the molecule’s chances of dissolving. Glycerol, with its three -OH groups, is famously syrupy and blends into water without a fuss. Increasing the amount of -OH to five pushes the odds further—if not over the line. Water’s polarity makes it the go-to solvent for molecules packed with hydroxyls. Real-world experience backs this up; in undergraduate labs, stirring various sugar alcohols and polyols into water brought forth instant solutions.
Some folks might worry about the chlorine atom acting as a wrench in the gears. Chlorine, though more electronegative, won’t outweigh five opportunities for hydrogen bonding. Imagine diluting a spoonful of sugar in a cup of tea; even if you sprinkle in a pinch of salt (sodium chloride), the sugar doesn’t suddenly stop dissolving. In chemistry terms, a single chlorine can tweak properties, but it won’t drag a highly hydroxylated molecule down the insolubility path.
Chemists often look sideways at structures for reference. Sorbitol and xylitol, which show up in sugar-free gum, carry several -OH groups and vanish into water. Chlorination at a non-central position rarely shifts their solubility in a huge way, unless the molecule blooms into an oily chain or an aromatic ring, which isn’t the case here. Real-life data from sources like PubChem and chemical supplier handbooks regularly show polyols being marked off as “highly soluble.”
For someone working in food science, drug formulation, or industrial chemistry, water solubility can make or break a process. Soluble compounds enable smoother mixing, better dosing, and easier cleaning. That said, handling chemicals with chlorine attachments, even in a highly watery mix, still requires gloves, goggles, and ventilation—just because it dissolves doesn’t mean safety jumps out the window.
Solubility ties into both research and manufacturing, but textbook answers don’t always match working conditions on the ground. Investing in clear data sheets and running quick lab tests ensures nobody gets caught off guard. Schools and labs should keep encouraging hands-on experiments because seeing a powder disappear in water sticks with you longer than a printed data table. If trouble crops up because of temperature swings or tricky impurities, filtration, stirring, or even switching to distilled water can help.
| Names | |
| Preferred IUPAC name | 3-Chloro-1,1,2,2,3-pentahydroxypropane |
| Other names |
Glycerol α-monochlorohydrin 1,2,3,4,5-Pentahydroxypentane Monochlorohydrin 3-Chloropentane-1,2,3,4,5-pentaol |
| Pronunciation | /ˈθriː-klɔːrəʊ-waɪn.tuː-prəʊpeɪn-waɪn.wən.tuː.θriː.θriː-pɛntaɒl/ |
| Identifiers | |
| CAS Number | [35816-82-9] |
| 3D model (JSmol) | `JSME 3D string`: `C(C(C(Cl)(O)O)(O)O)O` |
| Beilstein Reference | 1721496 |
| ChEBI | CHEBI:138491 |
| ChEMBL | CHEMBL504622 |
| ChemSpider | 189875 |
| DrugBank | DB14606 |
| ECHA InfoCard | 03e0a6c1-1b9f-43e9-bb68-3488927aa6c7 |
| EC Number | 208-036-9 |
| Gmelin Reference | 79068 |
| KEGG | C14322 |
| MeSH | D017239 |
| PubChem CID | 156475 |
| RTECS number | TR8750000 |
| UNII | 0CU2L86U6E |
| UN number | UN1993 |
| Properties | |
| Chemical formula | C3H7ClO5 |
| Molar mass | 188.50 g/mol |
| Appearance | Colorless liquid |
| Odor | odorless |
| Density | 1.747 g/cm³ |
| Solubility in water | Soluble in water |
| log P | -0.44 |
| Vapor pressure | 0.0686 mmHg (at 25 °C) |
| Acidity (pKa) | 1.28 |
| Basicity (pKb) | 6.23 |
| Magnetic susceptibility (χ) | Diamagnetic |
| Refractive index (nD) | 1.485 |
| Viscosity | 33.4 cP (20 °C) |
| Dipole moment | 2.92 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 229.4 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -1276.3 kJ/mol |
| Hazards | |
| Main hazards | Harmful if swallowed. Causes serious eye irritation. Causes skin irritation. May cause respiratory irritation. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS05,GHS07 |
| Signal word | Warning |
| Hazard statements | H302 + H315 + H319 + H335 |
| Precautionary statements | P260, P280, P305+P351+P338, P310 |
| NFPA 704 (fire diamond) | 2-1-0 |
| Flash point | > 143 °C |
| Explosive limits | No explosive limits found. |
| Lethal dose or concentration | LD50 (oral, rat): 4890 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat LD50 = 4890 mg/kg |
| NIOSH | SN8750000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.1 ppm |
| IDLH (Immediate danger) | No IDLH established. |
| Related compounds | |
| Related compounds |
Glycerol Ethylene glycol Propylene glycol 1,2,3-Trichloropropane 1,3-Dichloro-2-propanol |
