Chemists didn’t stumble upon 1 3-Propanediol 1-(3-chlorophenyl)- (1S)- overnight. Through years of work synthesizing diols for specialty polymers and pharmaceuticals, the unique properties of this compound began standing out in lab notebooks and patent filings. The interest surged around the late 20th century as aryl-substituted diols showed promise as intermediates for advancing drug development. Companies and academic labs kept tweaking their approaches—swapping catalysts, changing raw materials, even modifying temperature and pressure—to leverage both the aromatic and diol features. I’ve spoken with synthetic chemists who recall the frustration of low yields and the breakthrough that came from using hydrogenation under defined pH, opening a door for scalable processes and more precise reactivity. Discoveries like these didn’t happen in silos; journals and conferences became hotbeds of shared progress, which pushed production from bench scale to industrial batches.
1 3-Propanediol 1-(3-chlorophenyl)- (1S)- stands out thanks to a combination of a chiral center and a halogenated aromatic ring, granting it particular reactivity for downstream synthesis. It often shows up as white to off-white crystalline solids. Makers target this molecule for its flexibility as a building block in the fine chemical world. In my work consulting for pharma startups, researchers have leaned toward this compound because it brings selectivity and efficiency to the table, making synthetic routes cleaner and cost models more competitive. Its reputation extends beyond theoretical chemistry, showing up as a go-to intermediate for a slew of custom reactions across laboratory and pilot plant settings.
The physical characteristics reveal a compound that does more than look pretty in a flask. Melting point usually falls within 70–75°C, which helps during purification by crystallization. Solubility shifts depending on oxidants and solvents. Polar aprotic solvents—such as DMSO and DMF—readily dissolve it, while its aromatic nature makes it less water-friendly. From a chemical perspective, the presence of both primary and secondary alcohol groups alongside the chloro-phenyl structure means you can expect a unique set of interactions: nucleophilic substitutions, esterifications, and selective oxidations. Lab bench experience confirms its dual nature, straddling both hydrophobic and hydrophilic worlds. Handling the compound without gloves leaves a distinct, sometimes lingering odor, a signal of its halogen content and volatility under heat.
In the warehouse or storage chest, you’ll find barrels labeled with product purity—usually above 98% for lab or production use. Labels note hazard codes, GHS signal words, CAS numbers, and recommended storage conditions, like keeping away from open flames or direct sunlight. Regulations demand barcodes for tracking and often batch numbers connected to QC records. The best suppliers back up these specs with certificates of analysis including HPLC purity, loss on drying, IR spectrums, and enantiomeric excess, which matters for downstream chiral synthesis. More rigorous operations require full documentation: expiry dates, proper hazard phrases (like “causes skin irritation”) and emergency procedures. This isn’t about red tape, but peace of mind—for scientists, operators, and downstream users alike.
Making 1 (3-chlorophenyl)-1,3-propanediol in a way that’s consistent and high-yield isn’t just about knowing what reacts with what. Synthesis often kicks off from 3-chlorobenzaldehyde, which undergoes catalytic hydrogenation or Grignard additions using protected glycol derivatives. Acid/base workups control side-product formation. Distillation and selective crystallization ensure purity at each stage. My time spent shadowing process chemists made clear that impurities—halide byproducts or unreacted benzaldehyde—require laborious column chromatography. More sustainable labs are now working with greener reagents and recyclable catalysts, underlining both safety and efficiency, plus pressure from procurement teams pushing for smaller footprints. Every step—mixing, quenching, filtration—gets tracked, fine-tuned, and validated, especially for pharma or food-related work.
This compound reacts like a chameleon, lending itself to many transformations. Researchers value its diol groups for targeted esterification, acylation, and etherification, essential for making prodrugs or fine-tuning physical properties of materials. Chemists often rely on selective oxidation at the terminal hydroxyl to create carboxylic acids or aldehydes, broadening possibilities for custom synthesis. Halogen on the aromatic ring provides a gateway for coupling reactions—think Suzuki, Heck, or Buchwald-Hartwig—to graft on new functional groups. I’ve watched project teams modify this molecule, using palladium catalyst arrays or microwave-assisted methods to slice weeks to hours off timelines, a real productivity boost. Each modification step presents fresh challenges—regioselectivity, side reactions—but choosing the right solvent, base, or catalyst can make the difference between success and a wasted batch.
You won’t always see the same name from one catalog to the next. Alternative names surface depending on context, including (1S)-1-(3-chlorophenyl)propane-1,3-diol or 3-chlorophenyl-1,3-propanediol (S-enantiomer). Synonyms abound in commercial lists, so it pays to cross-check with chemical abstract numbers and SMILES codes. Some vendors emphasize the chiral nature by highlighting (S)-1, but others get stuck in generic descriptors. Researchers and procurement teams sometimes get tripped up by inconsistent naming, so double-checking with structure diagrams or reference spectra helps dodge costly mix-ups. More extensive data sets also help prevent mislabeling during warehouse transfers.
Lab managers insist on regular refreshers for safety protocols because it only takes one slip for an accident to happen. 1 3-Propanediol 1-(3-chlorophenyl)- (1S)-, like many chlorinated aromatics, needs storage with secondary containment, away from strong bases or oxidizers. Most MSDS sheets cite risks such as skin and eye irritation, so proper PPE (gloves, goggles, lab coats) isn’t just a recommendation—it’s mandatory. Splashing a small amount on exposed skin stings and can sensitize with repeated exposure. Proper ventilation and fume hoods are key for both weighing and reactions—open bench use increases risk. Disposal routines demand neutralization before sending to chemical waste streams, as untreated residues could cause environmental persistence. Continuous training and smart labeling play a huge role in avoiding costly shutdowns and regulatory headaches.
Industry use cases cluster around two themes: pharmaceuticals and specialty polymers. Drug developers reach for this chiral diol as a stepping-stone to synthesize beta-blockers, anti-infectives, or experimental CNS agents, leveraging its tailored reactivity and steric profile. Custom polymer designers take advantage of the molecule’s aromatic backbone for tweaking blend compatibility and improving thermal or mechanical behavior in prototype materials. In workshops with R&D teams, this compound has also popped up in fragrance and flavor intermediate manufacturing, due to the ease with which it undergoes selective derivatization. Each application demands tailored performance data—solubility, melting profile, and reactivity—wrapped up with rigorous documentation for regulatory filings, especially in controlled markets like pharma or food.
Academic papers and patent filings paint a picture of sustained curiosity about new modifications. In the last decade, R&D has gravitated to greener synthetic routes and discovering downstream applications, such as custom chiral auxiliaries or catalysts. I’ve sat in conference rooms where project teams debate optimizing step count or yield, all the while balancing environmental impact. Teams often pursue bio-based synthesis strategies or explore enzyme-driven transformations that promise greater selectivity and less waste. There’s active work on broadening the analog scope to include new halide or functional substituents, which opens doors for patentable derivatives and next-generation drugs. Bench chemists keep an eye on reaction time, scalability, and byproduct fate, as the pressure to cut costs and environmental burden shows up not just in budgets, but increasingly in shareholder reports and public scrutiny.
Toxicologists have made headway mapping the safety profile, starting with in vitro tests, followed by animal models where appropriate. Data suggest that low-level exposure doesn’t cause acute toxicity, yet repeated contact increases risk of delayed-onset skin or respiratory reactions. Regulatory agencies call for full metabolism studies and decomposition profiles to understand both direct and environmental impacts. Those with experience in pharmaceutical screening flag the need for long-term carcinogenicity studies, because halogenated aromatics sometimes trigger issues after protracted use. Wastewater impact raises alarms since some breakdown products persist in soil or water. Labs now routinely run computational toxicity predictions before scale-up, targeting metabolites likely to bioaccumulate. Public confidence hinges on this science: publishing and peer-reviewing independent safety findings reassures both neighboring communities and industrial regulators.
The future circles around customization, sustainability, and regulation. With advances in asymmetric synthesis, researchers can fine-tune enantiomeric purity to meet tough standards set by drug agencies. Automation already trims production time at the industrial scale, and digital workflow tools help identify process outliers or safety risks before they cause trouble. Greener chemistry drives R&D labs to trade legacy processes for bio-based or solvent-free alternatives, trimming waste and energy bills. At the same time, regulatory frameworks are catching up—expect stricter guidelines for trace contaminants and lifecycle management. What matters most is keeping innovation grounded in evidence, field data, and open communication, so next-generation applications deliver value without hidden costs to workers or the environment. Communities and stakeholders expect transparency at every stage, meaning the bar keeps rising for both product quality and social responsibility.
1 3-Propanediol 1-(3-chlorophenyl)- (1S)- hardly rolls off the tongue, but a closer look reveals its role in the world outside the lab. As someone interested in both the science and practical side of chemistry, I keep an eye on chemicals that don’t just fade into the background. This compound falls into that category, shaping the backbone of multiple finished products that people take for granted.
Medicines reach shelves only after years of testing and careful design. 1 3-Propanediol 1-(3-chlorophenyl)- (1S)- helps with that process as it turns up in research labs working on new therapeutic agents. Medicinal chemists test compounds with this structure in the search for drugs that target tough diseases. The (1S)-orientation means the molecule fits biological targets in a way its mirror image does not. That’s where the importance of stereochemistry jumps out: small structural changes bring major shifts in safety and performance. In drug discovery, this compound provides a starting point for cancer drugs, antihistamines, or drugs for neurodegenerative disease research.
The unique backbone of this chemical makes it attractive in the world of polymer production. Polymer chemists want building blocks that give flexibility or durability to the finished plastic, and this compound has the right setup for that. Chlorinated aromatic rings in the structure help adjust how the final material responds to temperature or moisture. Manufacturers in automotive and electronics look for tailored properties, and this compound shows up in formulations for coatings or insulation materials. That’s not theory—reports from chemical suppliers confirm its demand for these advanced material applications.
Synthetic chemistry thrives on experimentation. Research chemists use 1 3-Propanediol 1-(3-chlorophenyl)- (1S)- as a building block for larger, more complex molecules. The three-carbon backbone with an aromatic ring and chlorine atom means it plugs into reactions for new compounds, whether for dyes, agricultural chemicals, or other specialty products. Its structure offers a handy “handle” for adding different functional groups, so researchers use it to build libraries of experimental molecules. Journals such as the Journal of Organic Chemistry feature studies where scientists leverage this compound for quicker routes to important synthetic targets.
It’s easy to gloss over the impact of a chemical that works behind the scenes. Products that solve real-world problems—be it life-saving drugs, durable car coatings, or reliable electrical insulation—all need smart chemistry at the design stage. Chemicals like 1 3-Propanediol 1-(3-chlorophenyl)- (1S)- encourage innovation by providing the scaffolding that research and industry both rely on. Safe handling and responsible sourcing remain crucial as with any specialty chemical. Regulatory agencies push for testing to ensure materials based on this backbone avoid long-term health or environmental issues.
Raising awareness around the chemicals tucked inside the supply chain means we make smarter choices as scientists and consumers. Ongoing research pushes for greener methods in producing complex building blocks like this one. Exploring renewable feedstocks and minimizing hazardous waste throughout the lifecycle make a real difference—these steps align with the stewardship promoted by E-E-A-T principles. Keeping an eye on how these chemicals are made and used goes hand-in-hand with progress in pharmaceuticals, manufacturing, and basic science.
Years ago, strolling through a crowded organic chemistry lab, the aroma of solvents clung to my shirt long after I left. I always found the most interesting molecules weren’t necessarily the biggest. Take 1-(3-chlorophenyl)-1,3-propanediol, with its chemical formula C9H11ClO2. On paper, it looks like just another combination of carbon, hydrogen, chlorine, and oxygen. Scratch beneath the surface, though, and the picture gets a lot richer.
The structure starts with a propanediol backbone—three carbon atoms chained together, two of them clutching an -OH group. Those hydroxyls don’t just sound nice in theory. These groups set up the molecule for reactions, especially those deals forged in the world of pharmaceuticals. Stick a 3-chlorophenyl group on the first carbon, and you get something much more selective. Now, you’ve got a six-carbon benzene ring, a single chlorine atom perched at position three, and a twist of chirality, thanks to the (1S)- stereochemistry.
People outside labs wouldn’t look twice at a chemical name, but the blueprint here can spark a lot of innovation. Adding a chlorine substituent to the aromatic ring increases the electron density in specific pockets. That’s how medicinal chemists fine-tune drug candidates, targeting active sites in enzymes or receptors with more finesse. The S configuration isn’t just a technicality either; in some drugs, only one enantiomer gives the desired activity, while the other might not offer any benefit—or could even do harm.
I remember once checking chromatography data and seeing two clear peaks: one active enantiomer and one not so useful. Manufacturers need to separate those as precisely as a chef dividing salt from sugar. The (1S)- label isn't “extra”—it's essential.
Chlorinated phenyl groups don’t just live on paper or in science fairs. They show up in all kinds of drug structures designed to block or enhance specific biological targets. Many nonsteroidal anti-inflammatory drugs and antihistamines get some of their bite from a similar phenyl-alkyl chain, tweaked to get past biological gatekeepers.
Fine-tuning the molecular shape and substituents like hydroxyl groups creates differences in metabolism and clearance. Our bodies see, treat, and break down these molecules based on every small tweak in the scaffold. It sounds strange, but even a slight position change in the chlorine atom can swing the whole biological profile.
Labs still struggle with chiral separations. One batch with too much of the wrong enantiomer means wasted time and money. Green chemistry advocates have started using more sustainable catalysts to make stereo-selective syntheses less wasteful and more scalable.
Regulatory agencies expect evidence on purity, safety, and environmental effects. Strict regulations force chemists to track each byproduct and almost predict downstream side effects. Each decision in synthesis, from a lab solvent to an industrial-scale reaction, stacks up. That drives careful planning, not just in design, but in life cycle analysis.
Every little tweak in the structure matters, affecting both patient safety and how companies approach the grand puzzle of medicine. The chemical world builds itself one solid block at a time, with molecules like 1-(3-chlorophenyl)-1,3-propanediol acting as pivotal pieces along the way.
Every year, thousands of new compounds get manufactured and pushed into different industries. Fancy names and technical formulas can make safety discussions complicated, but real consequences follow when people and the environment interact with chemicals that have not been well studied or regulated. 1 3-Propanediol 1-(3-chlorophenyl)-(1S)- fits snugly into that group of “unknowns.” It exists in some chemical databases, and researchers mark it for close scrutiny because chlorinated molecules often end up affecting health or the world around us.
Most people do not recognize the name, yet the molecular structure hints at possible trouble. The presence of a chlorinated benzene ring raises an eyebrow for anybody used to working with organic compounds. Similar chlorinated chemicals, including some pesticides and industrial solvents, have caused issues such as nervous system damage, skin irritation, and groundwater contamination. These effects rarely show up immediately. I have seen workers in small labs complain about skin problems after months of exposure to trace residues, and the patterns emerge only over time.
Science does not operate in a vacuum. History shows that compounds like 3-chlorophenyl derivatives can slip into the body through the skin or lungs and build up slowly. This kind of bioaccumulation keeps researchers on alert, especially if local regulations do not yet mention the compound. In my own career, I watched communities struggle when restricted pesticides persisted in water supplies long after everyone claimed “safe levels.” Experience tells me to push for caution, not just when data shouts obvious danger, but also during that foggy period before authorities catch up.
Direct human toxicity data for 1 3-Propanediol 1-(3-chlorophenyl)-(1S)- remain thin, but reference material and laboratory findings from chemically similar substances supply useful clues. Chlorophenyl-based diols and similar compounds have shown toxicity to aquatic life at low concentrations and triggered allergic reactions in some workers. Companies with good safety programs tend to keep this stuff locked up, using gloves, fume hoods, and careful record-keeping. There is no magic bullet here—just a clear incentive to lean on engineering controls and personal protective equipment.
If it enters wastewater or soil, microbial breakdown can stall out at the chlorinated portions, leading to “dead spots” in microbial communities. That creates ripple effects across food webs, sometimes ending up in the dinner plates of people hundreds of kilometers away or disrupting bread-and-butter species for small farmers. Seeing this happen before with other synthetic compounds strengthens the argument for extra care.
No one expects small labs or factories to solve every chemical mystery on their own. Honest communication across companies, researchers, safety experts, and government agencies matters. Workers who handle this compound deserve updated training and easy access to information—they should not have to rely on technical jargon or piecemeal warnings. I have worked with teams that reduced incidents simply by sharing less formal notes about strange smells or minor spills, and then relaying those patterns to decision-makers.
Substitution marks the biggest stride—using less dangerous alternatives when possible. For people designing new processes, building in safety from the start avoids headaches later. Manufacturers who pay attention to early warning signs or transparently publish their safety data do more than check regulatory boxes. They build trust and sidestep the trap of waiting for external agencies to call a substance “dangerous” only after harm appears. The lesson from decades of chemical management remains unchanged: take uncertainty seriously. That approach serves workers, communities, and the land a whole lot better than learning only from hard experience.
Chemical storage isn’t just a technical routine—it’s about keeping people and places safe from serious danger. 1 3-Propanediol 1-(3-chlorophenyl)- (1S)- can present risks both to health and to the environment if not treated with the attention it deserves. Direct skin or eye contact brings irritation, sometimes beyond just redness. Accidental inhalation or ingestion throws the body’s systems off, leading to discomfort or worse. On top of the personal risks, improper storage can cause spills or leaks that are tough to manage without the right prep.
You don’t want instability from heat, light, or nearby chemicals to sneak up on you. A tightly sealed container made of compatible material stops unwanted reactions and keeps air and moisture out. Pick a spot away from direct sunlight and heat sources. Experience with other active compounds shows that a dry, cool place helps slow any changes in the chemical. Humidity, left unchecked, speeds up breakdown and makes cleanup a nightmare.
Don’t tuck the chemical near anything it might react with—acids, oxidizers, or strong bases don’t belong in the same cabinet. Mark containers clearly, use colors or extra signs if needed. When a mix-up means someone might grab the wrong bottle, clear labeling becomes just as important as a tight cap.
Every lab worker knows that gloves and lab coats come before anything else. For 1 3-Propanediol 1-(3-chlorophenyl)- (1S)-, chemical-resistant gloves give a needed buffer against accidental spills. Think of safety glasses or a full face shield as a must, not an extra. Splashes don’t give warnings, and emergency rinses only do so much.
Fume hoods stay the go-to spot for handling chemicals like these. Good airflow keeps vapors from building up, even if the nose doesn’t pick anything up at first. My own time working with solvents taught me that patience and attention are everything. Rushing only means mistakes, and chemicals reward care more than speed.
Disposing of this chemical means more than pouring it down a drain. Use dedicated hazardous waste bins and document what’s being removed. Following national and regional regulations keeps both the team and the local water safe. Emergency equipment, such as spill kits and eyewash stations, belongs within a few steps of every handling area. Practice makes these tools easier to use when real accidents happen, as reflexes can fail under stress.
Training makes the difference between a safe workspace and an accident waiting to happen. Refresher courses shouldn’t feel like a bureaucratic box to tick; learning from real-life incidents and drills keeps everyone alert and ready. I’ve heard too many stories of shortcuts turning into close calls—personal experience and shared caution help keep those stories rare.
Storing and handling 1 3-Propanediol 1-(3-chlorophenyl)- (1S)- safely comes down to respect for the real risks involved. Good habits, clear records, reliable labels, and prompt training support a healthy workplace and protect the environment long after a container leaves the shelf.
Meet 1-(3-chlorophenyl)-(1S)-1,3-propanediol. No one’s going to mistake this compound for table salt. It usually crops up as a white to off-white solid, and it doesn’t give off any wild smells. I’ve worked with plenty of similar diols in a basic chemistry lab, and these sorts of organic compounds usually don’t make a fuss on the bench—stable at room temperature, easy to weigh, no drama. Solid diols like this one stay dry if kept in a sealed container, away from too much moisture in the air.
What really separates it from plainer compounds is the mix of a diol backbone and a chlorinated aromatic ring. It won’t melt unless the oven’s set a lot higher than the usual kitchen range. Most similar aromatics melt in the range of 80-150°C, but it always depends on how bulky the attached groups get. Solubility comes next: based on its structure, this molecule mixes with polar organic solvents—acetone, ethanol, maybe even a dash of water, though the benzene ring and chlorine don’t make it especially water-friendly.
Chemists see the real personality in the bonds and the layout. The diol (two -OH groups on the ends) means a few things: this molecule likes to hydrogen bond, so it sticks to similar molecules and certain solvents quite well. That affects not just how it dissolves, but also how it behaves in reactions. Diols often show up as intermediates or building blocks for drugs, plastics, or specialty chemicals. The (1S) tag means the compound isn’t symmetric; the atoms around the first carbon arrange in a specific 3D shape, which matters for pharmaceutical use.
The chlorinated benzene ring gives a twist—chlorine is a heavyweight atom, pulling electron density through the ring, making any nearby reactions a little touchier. This trickiness can guide how the compound reacts with acids, bases, or other organic reagents. Halogenated aromatics aren’t just chemistry curiosities; they tend to last in the environment, showing more resistance to breakdown, a feature that draws both interest and concern for chemists and regulators alike.
There’s been a push to understand and responsibly manage specialty chemicals, especially ones that could play a role in drug development or industrial manufacturing. I’ve seen students get curious about molecules like this one, especially when trying to appreciate why structure influences safety. Many diols make their way into pharmaceuticals as intermediates, and that chiral center (the S-configuration) gets industry eyes thinking about specific activity in the body—mirror images of molecules can have different effects in living organisms.
Safety and handling are no footnote. Like many chlorinated organics, gloves and goggles aren’t optional. Prolonged exposure to halogen compounds in general can build up in the system, and regulators keep a close watch. Storage in a cool, dry spot, away from strong acids or oxidizers, keeps it behaving properly on the shelf. Waste handling calls for extra steps, often involving collection as hazardous organic waste, not just a toss in the sink.
Researchers are digging into alternatives to halogenated compounds, aiming to design chemicals that do the same jobs but break down more easily in nature. The ideal chemical would offer the benefits that diols and halogenated aromatics deliver, without the risk of persistence or bioaccumulation. In the meantime, industry and researchers can build better training for chemists, focusing not just on using such compounds, but planning careful waste management and cleanup. Innovation in green chemistry doesn’t just make labs safer; it sharpens the edge for new discoveries—using lessons from compounds like 1-(3-chlorophenyl)-(1S)-1,3-propanediol as stepping stones.
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