Chemicals like 1-Chlorooctadecane haven't just popped up overnight. Back in the days of rapid synthetic chemical evolution, chemists focused their craft on modifying naturally sourced alkanes. Fatty acid derivatives laid the groundwork. Chlorinating long-chain hydrocarbons started gaining momentum as industries chased surfactants and specialty waxes post-World War II. Researchers in the 1950s explored the chlorination of paraffins (paraffin chlorination became a favorite due to scalability and controllable results), branching out to specific chain lengths like octadecane. This allowed for more predictable melting points and performance in finished products. Over decades, as needs changed, so did the approach. Chemists shifted toward purer reactions, improved distillation, and less hazardous byproducts, but the backbone—long alkyl chains transformed with halogen groups—remained a steady presence in laboratories and production plants.
1-Chlorooctadecane is a straightforward molecule: take octadecane (an 18-carbon saturated hydrocarbon) and pop a chlorine atom on its primary carbon. As a result, it features a solid hydrocarbon backbone with a reactive halo group at one end. It's used as an intermediate in making surfactants and lubricants—filling a corner of the market where specialty chemicals are needed for tailored applications, such as antistatic agents or phase change materials. The specificity of the product comes directly from where the chlorine is attached; a primary chloride reacts quite differently from secondary or tertiary partners, so the precise configuration has direct consequences.
This compound shows up as a white, waxy solid at room temperature, with a modest melting point, usually around 30-32°C, and a boiling point north of 360°C under atmospheric pressure. Its solubility in water sits near zero, but it dissolves nicely in organic solvents, such as chloroform, ether, and hexane. The long hydrocarbon chain brings hydrophobic character, while the single chlorine atom at the terminal carbon tips the balance for reactivity. The molecule resists oxidation and reduction under mild conditions. Still, strong nucleophiles target the chloro group with enthusiasm, leading to a wide range of substitution reactions.
Buyers and handlers rely on technical sheets that spell out minimal purity, moisture content, melting point, halogen content, and residual unreacted octadecane or side-products. In those papers, purity often exceeds 98%. Labs keep a watchful eye on GC (gas chromatography) profiles, IR (infrared spectroscopy) confirmations, and sometimes NMR (nuclear magnetic resonance) checks to rule out unwanted isomers. On bottles and barrels, labels carry UN numbers (like UN1993), hazard symbols (danger: irritant, environmental hazard, depending on jurisdiction), safety recommendations, and the required chemical abstract service (CAS) number for traceability.
Producing 1-Chlorooctadecane relies on direct chlorination of octadecane, usually in the presence of UV light or heat, to encourage radical halogenation. While this approach sounds simple, high selectivity is tricky. To focus only on the terminal position (yielding the 1-chloro isomer, rather than a mix), process conditions get carefully optimized: mild temperatures, controlled rates of chlorine addition, and sometimes the use of radical initiators ensure fewer byproducts and cleaner output. The crude mixture undergoes vacuum distillation or recrystallization to isolate the pure compound, which ends up looking like a paraffin wax—neutral in odor and stable under storage, with only minor risk of darkening if left open to air and sunlight for too long.
Once in hand, this molecule opens the door to diverse transformations. The primary chloro group’s reactivity paves the way for SN2 (bimolecular nucleophilic substitution) chemistry—think swapping out chlorine for amines, alcohols, or thiol groups. These transformations build specialty surfactants, lubricant additives, antistatic agents, or even advanced phase-change materials for thermal storage. Strong bases strip the hydrogen next to the chlorine, forming terminal alkenes in elimination reactions—useful for further functionalization. The hydrocarbon portion can undergo modifications like sulfonation or oxidative cleavage, although reactions typically stick to the terminal group due to the molecule’s formidable length and chemical stability.
Scientists and manufacturers have called 1-Chlorooctadecane a host of names, sometimes leading to confusion. Synonyms include n-octadecyl chloride, stearyl chloride, and octadecane-1-chloride. On the shelf, international suppliers label it as Stearylchlorid, 1-chloro-n-octadecane, or even straight-up “C18 alkyl chloride.” Knowing the range of labels and product codes is essential for anyone looking to source, handle, or substitute the chemical in their workflow, as mix-ups between different chain-length chlorides can derail a synthesis or lead to unexpected properties in a finished product.
Anyone handling chlorinated hydrocarbons has to pay close attention to safety. This chemical may not be the most toxic in the class, but it can irritate skin and eyes, especially in higher concentrations or during heated processing. Laboratories require gloves, goggles, and solid ventilation—fume hoods aren’t optional. Spills clean up like other paraffinic compounds: absorbents, sealing, and safe disposal as chlorinated waste. Regulatory standards—like those set by OSHA, REACH in Europe, and various local agencies—stipulate restricted thresholds for occupational exposure. Fire risk exists due to the long hydrocarbon chain, even though its flashpoint sits higher than many common solvents; so, storage far from ignition sources and oxidizing agents reduces hazards.
Industries turn to 1-Chlorooctadecane for a handful of reasons. Surfactant manufacturers value its role as a building block for quaternary ammonium salts, cationic surfactants, and intermediates in textile and detergent formulations. Engineers use it as a slip agent in plastics or as a specialty lubricant for machinery, particularly where compatibility with other hydrophobic substances matters. In wax compounds, it finds its way into polishes and surface treatments. Some niche uses take advantage of its thermal properties, embedding the compound in phase change materials for temperature regulation systems or in certain drug delivery technologies where long alkyl chains improve biocompatibility.
Labs around the globe keep testing new ways to derive more value from 1-Chlorooctadecane. Some researchers probe greener synthesis methods, swapping gaseous chlorine for safer, in-situ halogen sources or bio-based starting materials. There's ongoing interest in catalytic routes, which can reduce byproducts and energy consumption. Chemists fiddle with the molecule to yield new surfactants with improved emulsification, lower toxicity, or enhanced antistatic properties. Materials scientists look at embedding the compound in new polymer blends, chasing tweaks in consistency or performance for electronics, coatings, or medical devices.
Safety data over the years show that, while the compound doesn't pose massive acute danger, it’s no stranger to environmental persistence. Chlorinated long-chain organics don’t break down quickly; they can bioaccumulate in aquatic systems and might sneak through conventional wastewater treatment. Studies observe low to moderate acute toxicity in mammals, primarily manifesting as mild skin and respiratory irritation at high concentrations. Chronic exposure hasn't triggered the level of concern associated with shorter-chain, more volatile chlorinated hydrocarbons, but the molecule’s stability and fat-solubility remind us to keep environmental release and worker exposure in check. Regular review of the latest toxicological data supports tighter controls and responsible use.
Looking ahead, 1-Chlorooctadecane’s story ties into larger trends in specialty chemicals. Regulation tightens, so greener processes and improved end-of-life degradability hold promise. Start-ups and legacy chemical players alike search for ways to build the same properties—hydrophobicity, reactivity at one end—using less persistent halogen atoms or even functional bio-based alternatives. If circular chemistry takes hold, redesigning molecules to fit new regulatory frameworks and shifting consumer attitudes could push research into functional, eco-friendlier analogues. AI-driven molecular discovery, better waste capture, and precision catalysis look set to shape a new chapter for long-chain alkyl chlorides. Still, the tried-and-true performance of 1-Chlorooctadecane keeps it firmly on the roster of specialty intermediates for now.
You might hear about 1-chlorooctadecane, often mentioned by chemists as a staple in industrial supply chains. It comes from the family of chlorinated hydrocarbons and features a long, 18-carbon backbone with a chlorine atom attached. At first glance, that probably does not make this substance sound like something the average person would care about. Dig in, though, and there’s more going on.
Manufacturers use 1-chlorooctadecane in several behind-the-scenes ways. In the world of lubricants, it often shows up as an additive that can reduce friction and wear, especially under tough conditions. It helps oils and greases last longer. Some rubber and plastic factories count on it as a key ingredient to help shape and process their products, enhancing the way raw materials slide through equipment. There’s no glamour in this work, but anyone who’s struggled with a squeaky hinge or brittle rubber can appreciate how these additives prevent headaches down the line.
If you’ve ever handled cable insulation or synthetic waxes, there’s a good chance an ingredient like 1-chlorooctadecane played a role. Factories turn to it as a chemical building block for surface coatings that protect wires and cabling from heat, moisture, and abrasion. Textile coatings sometimes draw on its properties to produce water-resistant finishes for clothes and tents. That touches real lives – no one likes soaked tents or shorted wires caused by poor insulation.
Chemicals with a long carbon chain and chlorine atom, like 1-chlorooctadecane, come with some baggage. Chlorinated hydrocarbons often raise eyebrows due to concerns about persistence in the environment and possible toxicity. People who work with this substance need to watch for skin or eye irritation. Studies on similar compounds show that they can accumulate in soil and water, potentially sticking around longer than most people would like. It’s easy to overlook these hazards if you do not spend time in factories or labs, but they matter every day to folks who make and use the products built from these chemicals.
Some cities and states now keep a close eye on how companies handle and dispose of these chemicals. Waste management rules set limits to keep them out of groundwater and off farm fields. Europe’s REACH regulations, for instance, require firms to gather more safety data before a chemical like 1-chlorooctadecane goes to market. Workers in chemical plants wear protective gear and follow training set out under OSHA and EPA standards in the US, or similar frameworks elsewhere.
Reducing reliance on these types of substances starts with innovation. Researchers continue to hunt for safer replacements in synthetic lubricants and coatings. Some companies use vegetable-based ingredients to achieve similar results without bringing extra environmental risk. Consumers and regulators want better labeling, clearer safety data, and a push for greener chemistry.
The story of 1-chlorooctadecane ends up looking like the bigger story about specialty chemicals. The stuff works well for tough industrial needs, yet its lifecycle—from creation in the lab to disposal—throws up hard questions. Transparency about what goes into the gear we use, the clothes we wear, and the shelters we rely on, lets people weigh benefits and risks, and decide where to draw the line.
1-Chlorooctadecane has always stood out during laboratory lessons. Picture a standard straight-chain alkane, in this case, octadecane, which runs for 18 carbon atoms. Swap out one of the hydrogens at the very first carbon and drop in a chlorine atom. This single change shifts its chemistry in surprisingly big ways. With each carbon holding two hydrogens and both terminals capped properly, you end up with the molecular formula: C18H37Cl.
People sometimes face confusion converting structural formulas into molecular ones. Take octadecane—C18H38 by default. Chop off one hydrogen since chlorine replaces it. Now it’s C18H37, add Cl. Chemistry textbooks always hammered home how every substitution slims the hydrogen count. It might seem basic, but overlooking it sends folks sideways in all sorts of chemical calculations.
The use of long-chain alkyl halides, such as 1-chlorooctadecane, keeps showing up in practical industrial work. These aren’t just lab curiosities; they serve real jobs. Their long hydrophobic tail sticks out in emulsions and coatings. That one inserted chlorine atom makes the molecule more reactive than its original alkane parent, which helps whether you’re building more complex organics or trying to tweak the surface qualities of a material.
Working with these compounds, I noticed their role in surfactant science. Have you ever tried breaking up oil slicks or stabilizing a paint before? Long straight chains latch onto oily stuff, while the chlorine tag opens a door for new reactions, such as nucleophilic substitutions or elimination. Researchers benefit from this flexibility—it makes synthesis shorter and more direct.
Not all chlorinated hydrocarbons make life simple. 1-Chlorooctadecane walks a middle line. Unlike smaller chlorinated chains, these long-chain halides present lower volatility, which means less inhalation risk, though skin contact still raises concerns. Chemists, environmentalists, and regulatory bodies look closely before putting substances like this into regular use, especially if wastewater management or soil contact factors in.
Chlorinated compounds have a reputation for stubborn persistence in the environment. Careless disposal can turn into a long-term contamination problem. Countries with strong environmental oversight push companies to recycle or carefully destroy halogenated waste. Modern setups often use closed systems during synthesis, collecting vapors and treating residues so communities nearby stay safe.
It’s worth mentioning the work toward greener substitutes. Chemists spend years exploring how to keep useful traits but lose the hazardous baggage. Some teams tweak synthesis by switching in less persistent leaving groups or developing catalysts that work at lower temperatures, which cuts down by-products. Young researchers often ask: Is this molecule indispensable, or can we swap it for something benign before production even starts?
Simple awareness—starting with the molecular formula—puts technical power in a chemist’s hands. Understanding those 37 hydrogens, 18 carbons, and solitary chlorine creates a domino effect, influencing how we manage safety, invent better processes, or even decide which chemicals earn a place in commercial manufacturing.
1-Chlorooctadecane isn’t likely to roll off anybody’s tongue. This chemical sees use in making things like surfactants, lubricants, and plasticizers. Some people won’t realize it, but it’s connected to products that show up at home or on the job. In chemical terms, it’s a chlorinated alkane with a long carbon chain. The industrial world likes it for its stability and how easily it blends with other ingredients. Still, getting past the technical stuff, people worry: what does this mean for health and the environment?
Most folks aren’t directly handling pure 1-Chlorooctadecane. Lab techs, plant workers, or people in the manufacturing world might get near it most. According to safety data, the chemical can irritate the skin and eyes if exposure goes uncontrolled. Breathing in vapors or fine mist can bother the respiratory system, though you’d have to really be in the thick of it for a while for more serious trouble to start. Experience in industrial settings has taught me the value of good gloves, face shields, and ventilation—skipping these shortcuts leads to regrets that show up later, especially with chemicals you can’t always smell or see coming.
People often worry about long-term problems like cancer or effects on organs. Right now, there’s not a big pile of evidence saying 1-Chlorooctadecane causes cancer or triggers other chronic illnesses for people who use it correctly and protect themselves. The EPA and EU’s chemical watchdogs haven’t flagged it as a confirmed carcinogen. That said, limited studies don’t guarantee safety—absence of proof is not proof of absence. Many times, the caution comes less from the compound itself and more from the way misuse or poor safety controls can let a hazardous situation develop. Chemical safety stories often share a theme: what you don’t know, or don’t bother to check, catches up with you over time.
This chemical sticks around for a while in soil or water. Once it leaks, it doesn’t break down quickly, so it can build up and possibly harm aquatic life. I’ve seen how accidents at industrial sites leave long-term headaches, from cleanup bills to angry neighbors. Responsible companies have learned this lesson—prevention costs way less than cleaning up a spill or fixing damaged reputation later. Spills, improper disposal, or lack of containment mean headaches for whole communities, not just workers inside the plant.
Simple changes cut risk before things get messy. Wearing protection isn’t optional; it’s the rule. Facilities need exhaust fans and regular air checks. Proper storage—think closed containers with good labeling—means fewer surprises. Training doesn’t look fancy on paper, but a workforce that understands what they’re handling always reports fewer injuries. For the average person, most risk disappears when companies follow these steps and when governments enforce them. Community awareness can help too. If people ask questions about runaway odors, or demand transparency after spills, everyone benefits. It takes a watchful approach—from companies, regulators, and local folks—to keep chemicals like 1-Chlorooctadecane in check.
Anyone who’s handled 1-Chlorooctadecane in a lab or warehouse knows its waxy texture and oily feel. This colorless to pale yellow chemical shows up most often in research and specialized manufacturing. Its long hydrocarbon chain signals that it won’t evaporate easily, but that doesn’t mean you can store it just anywhere. Plenty of people overlook simple, sensible rules when dealing with chemicals, which can lead to unsafe workspaces or wasted material.
Chemicals with a high hydrocarbon load tend to suffer when left in places that heat up or cool down too quickly. For 1-Chlorooctadecane, aim for a storage space between 15°C and 25°C (59°F to 77°F). A consistently cool, well-ventilated area keeps the product stable. Sudden exposure to heat nudges risk for decomposition or pressure build-up. I’ve seen containers swell and leak a slippery mess across concrete floors after someone left the bottle near a radiator. That creates a cleaning headache and puts people at risk for slips or skin contact.
It’s tempting to set chemical containers on a windowsill or a workbench for easy access, but that spells trouble. Light speed up reactions that most people never notice—discoloration, altered smell, or, worst of all, new byproducts. Wrap 1-Chlorooctadecane bottles in opaque bags or use brown glass containers if possible. Air and water, especially in humid climates, can get past a loose lid. A tightly sealed cap cuts moisture seepage, which prevents slow contamination and spoilage.
Sometimes I open a cabinet and find jars labeled with nothing but a chemical formula. That’s not helpful in a busy lab. Full labels, including the date received and any expiration milestones, cut confusion and avoid mixing up similar-looking compounds. It’s easier to catch storage mistakes before they turn into larger issues. A bit of extra care up front usually saves time and money later.
Some storage rooms get crowded, but that’s no excuse to let different chemicals mingle. 1-Chlorooctadecane should sit apart from strong oxidizers, acids, or anything reactive. Mixing these boosts the risk of fire or hazardous vapors, especially if a spill goes unnoticed. Common sense and a good inventory sheet shield against nasty surprises down the line. Safety Data Sheets (SDS) from reliable sources give more details on what to avoid pairing together.
Gloves, goggles, and lab coats sound basic, yet I’ve seen plenty of shortcuts. Spills might seem harmless until oily residues sneak onto your skin or clothes. Washing stations and absorbent pads nearby make cleanup simple and limit the chance of bigger accidents. Everyone on site, not just supervisors, should know the location of spill kits and understand emergency exit plans.
Old bottles can turn into hazards if forgotten at the back of a shelf. Workplaces following clear protocols for regular chemical disposal fare much better. Certified waste handlers know exactly how to process and neutralize 1-Chlorooctadecane without risking harm or fines. Tossing old chemicals in the trash or down the drain builds up long-term risks for waste systems and the environment.
Safe chemical storage doesn’t call for expensive systems or specialized rooms. Instead, practical habits—good labeling, cool and dry shelves, clear separation from incompatible materials, and proper training—do the heavy lifting. Paying attention every day keeps costs down and accidents far away.
1-Chlorooctadecane comes as a slightly viscous, colorless liquid with a faint, waxy aroma. Anyone who’s handled long-chain hydrocarbons in a lab knows the feel of oily compounds that coat glassware and hold on to the surface, almost like candle wax after melting. Its melting point hovers close to room temperature, usually reported near 20°C to 24°C, so the material flips between solid and liquid depending on how warm the room is. In practice, a bit of warmth turns crystalline flakes into a slick, clear fluid that pours much like mineral oil.
This compound’s density falls somewhere around 0.83 g/cm³ at standard conditions. That means it’s lighter than water but denser than a lot of low-molecular-weight hydrocarbons. It floats if poured into a beaker of water, which fits my own experiences working with similar molecules — you see an oily film slide across the surface, refusing to mix in. As for solubility, 1-chlorooctadecane barely budges in water due to its long non-polar tail. Standard lab tests show it’s more at home in organic solvents such as hexane or chloroform. This matters for folks mixing solutions or looking for a solvent system that keeps everything dissolved instead of separating.
The boiling point hits about 371°C, which makes sense for something with eighteen carbons in its chain. Common hydrocarbon solvents would have vanished from an open flask well before this one even gets close to boiling. That high temperature hints at stability under heat, though safety eyewear is non-negotiable if you ever run distillation with it. The melting point around room temperature can trip up beginners—if you store it in a chilly spot, you end up scraping, not pouring.
Anyone curious about the “feel” of 1-chlorooctadecane should know that repeated skin contact leads to mild irritation, nothing harsh but enough for gloves to become a habit. Labs use this molecule in organic synthesis, often for preparing surfactants or as an intermediate in more complex chemical reactions. Its long hydrocarbon chain helps lower the surface tension in mixtures, which means chemists use it in the prep for specialty materials that need just the right balance of hydrophobic and hydrophilic regions.
A slip-up seen before: using ordinary glass droppers or pipette bulbs. Over time, chlorinated hydrocarbons put stress on certain plastics, leading to small cracks and losses of sample. Switching to all-glass tools and keeping lids tightly closed has spared many a sample from evaporation and contamination.
Long-chain chlorinated hydrocarbons do not vanish quickly in the environment. Slow breakdown rates have drawn scrutiny, especially in communities living close to chemical plants. This class of compounds can persist in soil and water, so engineers and lab workers follow best-practice handling and disposal guidelines set by regulatory agencies like the EPA. Storing the material in amber glass bottles away from direct sunlight maintains stability and safety for long periods.
Researchers and industry professionals who know their way around environmental surveys make a point to track emissions and leaks from storage containers. Even a small release can linger, so the responsibility for careful storage never gets old.
| Names | |
| Preferred IUPAC name | Chlorooctadecane |
| Other names |
Chlorooctadecane
n-Octadecyl chloride Stearyl chloride 1-Chlorooctadecan Octadecyl chloride |
| Pronunciation | /ˌklɔːroʊ.ɒkˈteɪ.deɪn/ |
| Identifiers | |
| CAS Number | 112-88-9 |
| Beilstein Reference | 1718734 |
| ChEBI | CHEBI:34410 |
| ChEMBL | CHEMBL510484 |
| ChemSpider | 13865223 |
| DrugBank | DB16056 |
| ECHA InfoCard | EC Number 203-444-5 |
| EC Number | 214-482-9 |
| Gmelin Reference | 8586 |
| KEGG | C14262 |
| MeSH | D017355 |
| PubChem CID | 12409 |
| RTECS number | RN0130500 |
| UNII | Q2M7I4H6L9 |
| UN number | UN1993 |
| CompTox Dashboard (EPA) | 'DTXSID8020203' |
| Properties | |
| Chemical formula | C18H37Cl |
| Molar mass | 320.00 g/mol |
| Appearance | White to light yellow solid or liquid |
| Odor | Odorless |
| Density | 0.851 g/mL at 25 °C (lit.) |
| Solubility in water | Insoluble |
| log P | 10.14 |
| Vapor pressure | 0.000022 mmHg at 25°C |
| Acidity (pKa) | ~50 |
| Magnetic susceptibility (χ) | -88.0e-6 cm³/mol |
| Refractive index (nD) | 1.434 |
| Viscosity | 4.427 mPa·s (20°C) |
| Dipole moment | 2.60 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 560.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -353.5 kJ·mol⁻¹ |
| Std enthalpy of combustion (ΔcH⦵298) | -11920.8 kJ/mol |
| Pharmacology | |
| ATC code | D14AB06 |
| Hazards | |
| Main hazards | Harmful if swallowed, causes skin and eye irritation, may cause respiratory irritation. |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | Hazard statements: H315, H319, H335 |
| Precautionary statements | Precautionary statements of 1-Chlorooctadecane are: "P264, P270, P273, P301+P312, P330, P501 |
| NFPA 704 (fire diamond) | 1-1-0 |
| Flash point | 152 °C |
| Autoignition temperature | 265 °C |
| Lethal dose or concentration | Lethal dose or concentration (LD50/LC50) data for 1-Chlorooctadecane: "LD50 (rat, oral) > 5000 mg/kg |
| LD50 (median dose) | LD50 (median dose): Rat oral >5 gm/kg |
| NIOSH | CY9270000 |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.1 |
| Related compounds | |
| Related compounds |
1-Bromooctadecane
1-Iodooctadecane Octadecane Stearyl alcohol |
