Chemists in the early 20th century actively sought out simple chlorinated alkanes, leading to the discovery of compounds like 1,6-dichlorohexane. Driven by the boom in industrial chemistry, this compound offered a reactive yet manageable bridging molecule for research and manufacturing. As scientists learned more about alkyl halides, they found that the dichlorohexane variant created reliable building blocks for polymers and specialty chemicals. Its adoption mirrored broader trends in organic synthesis — using small, well-understood molecules to shape larger, more complex structures. Lab manuals from old chemistry courses often reference it as a foundational reagent, I recall using it in early polymer chemistry classes where its stability made it much more forgiving than shorter-chained or more heavily halogenated oils.
1,6-Dichlorohexane shows up as a colorless to pale yellow liquid that gives off a faint, sweet chemical odor. It fits into the larger family of saturated chlorinated hydrocarbons, with two chlorine atoms anchoring the terminal spots on a six-carbon backbone. A versatile chemical, it pops up across labs, manufacturing sites, and even agrochemical development thanks to its role as a chemical intermediate. Various suppliers produce it to lab purity or industrial-grade standards, so it’s not just a specialist’s tool. Labels and safety sheets often warn about handling precautions, reflecting lessons learned from decades of experience with organochlorine exposure.
With a molecular formula of C6H12Cl2 and a molecular weight a shade past 155, 1,6-dichlorohexane blends moderate volatility with a boiling point of about 228 °C. Its density sits close to 1.08 g/cm³, just enough to float or sink depending on what else ends up in the flask. The compound doesn’t dissolve in water, but it readily mixes with ethers, alcohols, and simple hydrocarbons, which helps it slot into all sorts of preparations. Chemically, the molecule acts as a competent alkylating agent. In the lab, those two terminal chlorines respond well to nucleophilic substitution, making the compound useful for building up more complex organic frameworks.
Producers assign clear-cut parameters for this compound on every drum and bottle. Typical specs focus on purity, water content, acidity as HCl, and residual organics, often demanding assay values of 98% or above for research purposes. GC-MS and NMR analysis confirm the structure and high grade. Labels include the usual hazard pictograms: corrosive, irritant, and environmentally hazardous, underscoring the need for gloves and fume hoods. Transport rules line up with other chlorinated solvents, featuring UN numbers, hazard classes, and special codes for bulk or sample-size shipments.
Producers usually make 1,6-dichlorohexane via chlorination of hexane or by treating 1,6-hexanediol with hydrochloric acid. Both routes push for high conversion rates and selectivity, since over-chlorination or incomplete reaction leads to all kinds of headaches. Industrial-scale synthesis uses controlled conditions — closed reactors, chilled condensers, and rigorous waste treatment — to cap emissions and boost yield. In the lab, careful distillation follows the main reaction; it’s a process that takes time and patience, often requiring more than one pass to reach analytical purity. I've personally run small-scale reactions and always appreciated the delayed boiling and distinctive layering during extraction, which signals a clean prep.
Having those two chlorines on opposite ends opens the door to a world of substitutions. Nucleophilic species, such as primary amines or alkoxides, replace the chlorides cleanly under the right conditions, resulting in diamines, diethers, or longer-chain macrocycles. Chemists exploit its symmetrical nature to crosslink polymers or to introduce functional groups that lead to specialty compounds — lubricants, surfactants, or even responsive hydrogels in biotech. A single bottle can support dozens of research paths, each relying on the predictable snap of a carbon-chlorine bond under the tug of a strong nucleophile.
Depending on the context, manufacturers, or regulatory databases, the compound goes by several monikers. Most in the industry stick to "1,6-dichlorohexane." Some catalogs add "hexamethylene dichloride," and less commonly, users call it "hexane-1,6-dichloride." Its CAS number — 2163-00-0 — shows up on global safety and shipping lists. Anyone sourcing the substance needs to be alert to the different synonyms, especially if searching through international inventories or regulatory notices.
Safe handling of 1,6-dichlorohexane depends on rigorous training and respect for organochlorine risks. It can irritate the skin, eyes, and respiratory tract, and repeated exposure sometimes leads to more serious systemic effects. Proper ventilation, gloves, and splash-proof goggles end up as daily necessities instead of optional extras. In my earlier research jobs, spill kits and emergency showers always stood nearby anytime we cracked open a bottle. Regulatory agencies restrict its release to the environment, placing tough rules on waste handling and storage to keep chlorinated volatiles out of air and groundwater. Safety data sheets warn against both acute and chronic effects, which keeps new generations of chemists on alert.
1,6-Dichlorohexane finds its main footing as a crosslinking agent for polymer synthesis, where it bridges functional groups on long-chain molecules to create robust plastics and elastomers. The electronics industry taps it for specialty coatings and insulating layers. Its reactivity creates starter blocks for pharmaceuticals—just two or three well-controlled exchanges can build up complex intermediates for active ingredients. Agrochemical research uses it to tailor new pesticide scaffolds, working with its chain length and substitutable ends. Its applications expand with every discovery in organic synthesis, and chemists continue to count on its reliability for foundational work in fields as diverse as material science and medicinal chemistry.
Research on 1,6-dichlorohexane these days moves well beyond basic reactivity. Scientists harness it as a template for making functionalized polymers, experimenting with novel membrane materials, microcapsules, or even smart hydrogels for targeted drug release. I've seen recent academic work pushing its use into advanced supramolecular assemblies — things like molecular machines and responsive gels that react to heat, light, or pH. R&D teams also keep reshaping the main synthesis process, aiming for greener, more selective reactions that produce less hazardous waste. Modern analytical techniques — high-resolution NMR, mass spec, automated titration — make tracking every byproduct much easier, trimming down environmental impact and cost. Many students start out with simple substitutions on this molecule and move to more advanced concepts from there, making it a staple of core synthetic chemistry training.
Toxicologists keep a wary eye on chlorinated additives like 1,6-dichlorohexane. Animal studies point to potential for dermal and respiratory irritation, and accidental exposure in industrial settings can spark headaches, nausea, or worse when left unchecked. Chronic exposure remains a topic for ongoing debate, although heavy reliance on safety equipment and closed systems minimizes risk for most workers. Environmental toxicology flags the risk to aquatic life due to its persistence and moderate bioaccumulation. Global databases — ECHA, EPA, PubChem — logging incident reports, lab test results, and incident studies now guide updated handling protocols. Better toxicity screening pushes manufacturers to reassess process design and inform customers more thoroughly, shifting the focus toward transparency and stewardship.
Looking ahead, the future of 1,6-dichlorohexane connects deeply with industry’s push for greener chemistry. Researchers evaluate bio-derived hexanediol for conversion, reducing reliance on petroleum feedstocks. Advances in catalysis and flow chemistry also promise cleaner, faster routes with less energy wasted and fewer byproducts to dispose of. Polymer science keeps searching for new crosslinkers and process modifications, with 1,6-dichlorohexane often serving as the benchmark for comparing new alternatives. Regulation may tighten as more is learned about organochlorine’s long-term effects, yet demand sticks around as long as specialty chemicals, durable plastics, and advanced coatings need versatile, well-characterized intermediates. Experience in processing and handling will travel forward, updated by results from today’s research and new safety data, keeping both innovation and risk reduction at the core of chemical manufacturing.
Step into a chemical plant, and you may hear talk about 1,6-dichlorohexane. This compound quietly supports the work behind plastic products, specialty coatings, and nylon. In my time researching materials for engineering firms, I noticed 1,6-dichlorohexane pop up most in the world of nylon-6,6. Chemists need it to create the hexamethylenediamine building block. Without this piece, you don’t get strong, heat-resistant nylon car parts, or the resilient carpet fibers found in so many homes and offices.
In plastics, the ability to tweak a polymer’s structure becomes a huge advantage. Here, 1,6-dichlorohexane offers a way to add length or durability by creating linkages you just can’t get with other chemicals. Process engineers often value an efficient route to stronger, more weatherproof materials. They use 1,6-dichlorohexane for exactly this reason, particularly when aiming for custom solutions and applications outside of mass-market choices.
Few people think about industrial synthesis. Yet every cell phone, auto interior, and appliance relies on reactions involving chemicals like 1,6-dichlorohexane. This molecule brings two chlorine atoms spaced out by six carbon atoms, which makes it a solid candidate for adding chains or branches to polymers. The reactivity of the terminal chlorine atoms means manufacturers can build bigger, tougher materials with fewer byproducts. I’ve seen small mistakes in reaction control snowball into costly production delays, so having stable intermediates makes a real difference to the people running the show.
Pharmaceutical researchers have experimented with 1,6-dichlorohexane while testing new drugs, mainly for its properties as a linker. I spoke to a team in medicinal chemistry at a university that appreciated its “leggy” backbone—just long enough to serve as a bridge in molecular structures, but not bulky enough to slow down a reaction. For research teams looking at new cancer drugs, the fine control over molecular shapes and bindings helps nudge a promising compound into something worth scaling.
Nobody should ignore the hazards tied to chlorinated hydrocarbons. I remember touring a facility where the storage protocols for 1,6-dichlorohexane sat right up there with the volatile solvents. Prolonged exposure affects the nervous system and breathing over time. Strict ventilation and regular staff training in proper handling gear often keep everyone safe. Recognizing these risks matters, as regulatory scrutiny around production and waste treatment grows every year.
On the environmental side, runoff or improper disposal leads to water contamination. Some plants recapture any emissions with scrubbers or convert unused material to less hazardous forms before it ever touches a drain. The chemistry community continues to search for greener alternatives and waste-reduction tactics, but the simplicity and cost-effectiveness of 1,6-dichlorohexane keep it in circulation.
Some manufacturers look at biosynthetic routes or less toxic reagents. While biotech solutions promise cleaner outputs, the scale and price often lag behind what the established supply chain delivers. Research funding aims at enzymes and fermentation-based options, but wide adoption takes time. In the labs and plants where 1,6-dichlorohexane gets used daily, real improvements often start with small changes: switching to closed systems, updating personal protective equipment, and fine-tuning recycling processes.
Progress in chemistry isn’t just about new discoveries; it leans heavily on the constant push for smarter, safer, and cleaner practices. 1,6-dichlorohexane may not grab headlines, but the work that happens around it shapes the modern world.
1,6-Dichlorohexane builds plastics, pharmaceuticals, and some specialty coatings. This clear liquid doesn’t really give off a strong smell, so there’s a false sense that it’s harmless. Dig deeper into its profile and it quickly becomes obvious why nobody should take it lightly. This substance can irritate the skin, eyes, and lungs. If you breathe in vapors over time or accidentally splash it around, you’re looking at chemical burns, headaches, dizziness—possibly more severe long-term problems. That’s not theory. Get a bit careless and the risks are real. I learned early on by watching a colleague rush clean-up and end up with a rash that took weeks to go away.
Gloves and goggles are non-negotiable. Nitrile gloves stand up better than standard latex, especially because 1,6-dichlorohexane soaks through some materials faster than expected. Go with a lab coat or chemical apron—cotton clothes alone won’t cut it since any drips can quickly seep through. For splashy tasks or transfers, a face shield helps a lot. I always keep my goggles clean; smudges might not seem like much until something goes flying and you’re suddenly blinking away a stinging mess.
Any work with this chemical belongs inside a well-maintained fume hood. Relying on a cracked window or a cheap desk fan might move air around, but it does nothing to stop exposure. Years ago, my lab ran side-by-side exposure monitors: the numbers dropped by 90% inside a hood. Labs without ventilation upgrades risk breathing in low levels over weeks or months, which shows up as headaches, fatigue, and in some studies, even liver trouble.
Never toss 1,6-dichlorohexane on a crowded shelf or near heat. This stuff starts to break down above normal room temperatures, giving off more vapors and building up pressure in sealed containers. Use tight-fitting, hazard-labeled bottles. I keep mine in a flame-proof cabinet away from anything acidic or oxidizing. In one shared space, we nearly had an incident when someone stored this compound next to bleach—luckily someone caught it before work began that day.
Spill kits stocked with absorbent pads and neutralizers hang near every bench in my lab. Small puddles get soaked up, sealed in chemical-waste bags, and recorded in the logbook. For bigger spills, don’t improvise—evacuate and call trained responders. Disposal matters too. Pouring leftovers down a drain or mixing into general waste adds up to costly fines and environmental hazards. My group uses an outside vendor for disposal and reviews the log once a month. This habit catches careless shortcuts before they set in.
No one gets to handle anything like 1,6-dichlorohexane in my lab without proper training. That means drills, refreshers, and hands-on walkthroughs. Textbook knowledge feels safe, but muscle memory during a stressful moment can be the difference between a close call and a hospital trip. Building a steady, safety-first culture encourages people to speak up and double-check. That’s paid off plenty of times—one overlooked glove or broken storage bottle, caught in time, spares the whole team a lot of trouble.
Some labs have started switching to less toxic substitutes where it makes sense. Substitution works in some syntheses, and it’s a huge step forward for long-term health. Still, industries move slowly. Until then, each person working with this chemical needs to take responsibility—protective gear, clear labeling, and the mindset that a shortcut isn’t worth the risk. Everyone I know who works with 1,6-dichlorohexane can point to close calls. The ones who stay healthy treat safety as just another part of the job, built into every pour and transfer, every single day.
1,6-Dichlorohexane carries the chemical formula C6H12Cl2. Just counting atoms doesn’t capture why this structure matters. Picture a hexane backbone: six carbon atoms in a string, each carbon linked by single bonds, just like the skeleton in countless molecules found throughout industry and research. Slap a chlorine atom on both the first and sixth carbon, swap out two hydrogens, and you have 1,6-dichlorohexane. That makes it a dihaloalkane, with just two points open for reaction. This design is more than a chemical curiosity—it delivers unique reactivity and shapes how it gets used.
Chemical formulas might look like alphabet soup, but every letter and number signals how a molecule will behave. C6H12Cl2 lines up as a key intermediate in polymer chemistry, thanks to those reactive chlorines dangling at each end. In my own experience in college labs, dichloroalkanes like this were go-to building blocks for linking molecules together. Unlike some slick, high-profile reagents, it does its job quietly, delivering reliability in synthesis. Pick up a bottle, pop the cap, and you can almost smell the industrial world behind it—synthetic lubricants, plasticizers, everything needing a strong, flexible carbon chain with reactive handles.
Industries tapping into chlorinated hexanes often chase durability or chemical resistance for specialty plastics. The way chlorines anchor themselves to the carbons gives manufacturers an edge; it helps graft different properties onto polymer chains, nudging performance up for wiring insulation or high-end tubing. Students and bench chemists turn to these molecules when they need a simple path to more complicated targets, using classic nucleophilic substitution reactions to swap in functional groups. C6H12Cl2 stands out because the ends are reactive, but the core—the hexyl backbone—offers flexibility and stability at the same time.
The presence of chlorine flags a safety issue. Halogenated organics don’t just vanish into thin air. Mismanagement can lead to persistent pollution, a problem that cropped up in communities around manufacturing hubs. Facts back that up; organochlorines are slow to break down and tend to build up in ecosystems. Researchers found traces of related compounds in soil and water near chemical plants, and it’s no secret that some—though not all—can mess with wildlife and human health.
There’s pressure to handle these chemicals with care, both to protect workers and limit harm to the surrounding environment. Factories now stack on scrubbers and solvents to catch emissions. In our university labs, strict protocols cut down on accidental releases—closed containers, fume hoods, and smart waste disposal were all non-negotiable. Progress means digging up greener alternatives for some uses, but so far, the unique shape of 1,6-dichlorohexane keeps it in rotation for certain advanced materials. Responsible use, clear labeling, and attention to the risks keep people and the planet safer without shutting the door on the molecule’s benefits.
Anyone dealing with 1,6-Dichlorohexane should stop and think about what’s really at stake. This chemical isn’t the sort you set on a shelf and forget. You need to respect the risks—both for your own best interest and for those working around you. 1,6-Dichlorohexane brings fire dangers, harmful vapors, and can burn your skin or irritate your lungs. These hazards stick around unless you take storage seriously.
After a few years working in industrial labs, I learned that cutting corners creates problems. A supervisor once stashed a drum of chemicals near a heat vent, and the next day, we caught a strong, unpleasant smell. That drum, sweating and warped, reminded everyone: heat doesn’t just threaten the product. Fumes build up pressure, leak, and someone gets hurt. Storing 1,6-Dichlorohexane means finding a cool, dry spot, away from direct sunlight or machinery that radiates heat. Think in terms of temperature control. Under 25°C works best, with steady monitoring—not “set it and forget it.”
Vapor-tight containers play a direct role, too. If the seal isn’t perfect, you’re breathing in fumes, and that’s not smart or healthy. Polyethylene drums, steel containers with tight lids and non-rusting linings, or specialty solvent cabinets? All have value if sealed right. I’ve seen labels fall off after a spill and watched the panic ripple through a room afterwards. Use solvent-resistant labels, with clear hazard info—no lazy handwriting or half-peeled stickers. Mislabeling can send someone to the ER, so don’t compromise on that detail.
Long-term storage in a basic storeroom never cuts it. Dedicated chemical storage rooms or cabinets, equipped with ventilation and spark-proof lighting, drop the odds of a fire. I’ve heard folks say they’ll take care once the inspection date rolls by, but hazards don’t check the calendar. Store far from break rooms, kitchens, or any food prep areas. Food surfaces collect vapors, and someone’s lunch gets a chemical tang. A simple line of separation keeps accidents down and people healthy.
One lesson I picked up over the years: nothing beats a spill kit within arm’s reach. Personal stories from colleagues across chemical plants all make the same point. A cracked lid leaks faster than most expect. Granular absorbents, chemical-grade gloves, splash goggles—these need to be closer than the nearest locker. If you spot a leak or the smell grows strong, immediate cleanup stops a small error from becoming a big disaster. Relying on ventilation alone isn’t enough—containment gear and cleanup plans do the hard work. Training for everyone, not just supervisors, sets the tone. People make fewer mistakes when they know what to do, and mistakes with 1,6-Dichlorohexane rarely forgive.
Stories spread fast—like the warehouse manager who ignored a drippy container, hoping it would sort itself out until the fire alarm screamed. These tales matter because they remind us chemical safety demands steady effort, not just checklists. Building a habit of regular checks, setting clear boundaries around storage spaces, and never reusing containers for other chemicals reduces risk. 1,6-Dichlorohexane pushes us to act with care and to teach others why shortcuts just aren’t worth it. Responsible storage offers one real upside: people go home safe, and the boss doesn’t get late-night phone calls about “unplanned incidents.” Facts, experience, and a little common sense create safer workdays, every day.
A lot of industrial products come with names nobody talks about outside chemistry class. 1,6-Dichlorohexane is one of those. You’ll see it used in making plastics, specialty rubbers, and certain coatings. It’s meant for manufacturing—most people on the street don’t handle it, but people in chemical plants probably do.
I’ve met workers in plants who wear thick gloves and filtered masks every day. There’s a good reason. 1,6-Dichlorohexane can get through your skin, and breathing its fumes isn’t a smart move. Studies done on rats point toward toxic effects on the nervous system, liver, and kidneys when exposure levels go up. Even though specific reports in humans are rare, most occupational safety agencies have flagged it as something that can cause trouble with enough contact.
A single whiff or splash probably won’t send someone to the hospital, but repeated handling cranks up the risk. Folks who worked around it for years showed skin peeling, headaches, and slow, ongoing irritation. The Centers for Disease Control and Prevention highlight the chemical as a contact hazard and say to avoid inhaling vapors. It easily passes into the body because it evaporates at room temperature.
Factories that use 1,6-Dichlorohexane run into one big problem: chemical leaks don’t always stay put. This chemical doesn’t break down quickly. Once dumped or spilled, it can slide into soil and drift through groundwater. A study by the U.S. Environmental Protection Agency found that chlorinated alkanes like this one show up in groundwater near manufacturing sites long after leaks.
Fish and bugs deal with it in their own ways, but 1,6-Dichlorohexane doesn’t go away fast. Over time, even small releases can build up and hurt aquatic life. The chemical affects living creatures lower in the food chain, making its way up to fish and birds that eat them. The environmental risk isn’t always dramatic and immediate, but it sticks around.
Keeping people safe starts with how it’s handled at factories. I’ve seen real progress where companies invest in sealed systems. Workers get training that goes beyond videos—they rehearse accidents and practice cleanups together. Emergency showers and proper ventilation help lower the risk for those handling it.
On the waste side, collection and treatment systems keep leaks from making their way into rivers. Factories that reuse or properly incinerate left-over chemicals put up less risk to ground and water. Some countries push for alternatives, nudging companies to swap out harmful chemicals where possible.
Personal responsibility matters, but oversight works better when governments check that companies play by the rules. Sites with a history of leaks get regular inspections, and good reports show fines help keep companies on their toes. When workers know why the rules exist, safety habits take root and last longer than any sign stuck to the wall.
1,6-Dichlorohexane sounds like science fiction, but it’s a steady presence in industrial chemistry. Where safety breaks down, people and nature pay the price over years. Real progress shows up in well-trained staff and strict rules that stay enforced. Nobody’s asking for miracles—just a common sense approach built on facts and hard-earned experience.
| Names | |
| Preferred IUPAC name | 1,6-dichlorohexane |
| Other names |
1,6-Dichlorohexane
Hexamethylene dichloride Hexane, 1,6-dichloro- NSC 27092 |
| Pronunciation | /ˌwʌn,sɪks-daɪˌklɔːroʊˈhɛkseɪn/ |
| Identifiers | |
| CAS Number | 2162-98-3 |
| 3D model (JSmol) | `CCCC(Cl)CCCCl` |
| Beilstein Reference | 82652 |
| ChEBI | CHEBI:44465 |
| ChEMBL | CHEMBL15323 |
| ChemSpider | 10650 |
| DrugBank | DB08763 |
| ECHA InfoCard | 03ee2eaf-7b79-4f12-9698-506a76f2a15d |
| EC Number | 202-658-0 |
| Gmelin Reference | 104141 |
| KEGG | C01782 |
| MeSH | D003976 |
| PubChem CID | 12476 |
| RTECS number | MO2625000 |
| UNII | W38T1Y52RZ |
| UN number | UN2526 |
| Properties | |
| Chemical formula | C6H12Cl2 |
| Molar mass | 187.07 g/mol |
| Appearance | Colorless to pale yellow liquid |
| Odor | Odorless |
| Density | 1.09 g/mL at 25 °C(lit.) |
| Solubility in water | Insoluble |
| log P | 3.6 |
| Vapor pressure | 0.09 mmHg (25°C) |
| Acidity (pKa) | > 15.2 |
| Magnetic susceptibility (χ) | -7.92e-6 cm³/mol |
| Refractive index (nD) | 1.464 |
| Viscosity | 2.25 mPa·s (25 °C) |
| Dipole moment | 2.11 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 380.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -204.8 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -3896.9 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS07 |
| Signal word | Warning |
| Hazard statements | H302+H312+H332, H315, H319 |
| Precautionary statements | P210, P261, P280, P301+P312, P305+P351+P338, P304+P340, P308+P313, P501 |
| NFPA 704 (fire diamond) | 1,2,0 |
| Flash point | 94 °C (201 °F; 367 K) |
| Autoignition temperature | 285 °C |
| Explosive limits | Explosive limits: 0.9–6.4% |
| Lethal dose or concentration | LD₅₀ oral rat 2500 mg/kg |
| LD50 (median dose) | LD50 (median dose): 3,540 mg/kg (rat, oral) |
| PEL (Permissible) | Not established |
| REL (Recommended) | 0.5 ppm |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
1,6-Dibromohexane
1,6-Diiodohexane 1,6-Difluorohexane 1,6-Dichlorohexene 1,2-Dichloroethane 1,4-Dichlorobutane Hexane |
