1-Chlorooctane: A Grounded Look at Its Role and Realities
Historical Development
1-Chlorooctane entered commercial catalogs over a century ago, well after its closest relatives, the simple alkyl chlorides, found favor as laboratory reagents and synthetic intermediates. Once researchers unlocked the methods for substituting a halogen onto aliphatic hydrocarbons with consistency, the blueprint for producing chlorinated straight-chain molecules like 1-Chlorooctane followed quickly. In those early days, no one gave much thought to its future roles as a link in petrochemicals or as a handy intermediate. The slow adoption had more to do with limited applications paired with the cost of raw materials. Older synthesis routes—using phosphorus trichloride, thionyl chloride, or hydrogen chloride gas on octanol—set the pattern, but product isolation and scale-up seemed tricky for a while. By the 1960s, better chemical engineering and the spread of commodity-scale reactors made 1-Chlorooctane a staple in portfolios of European and American chemical houses. I see the company archives showing it appeared in catalogs with an eye toward specialty synthesis rather than mass market use, echoing its relatively niche but quietly persistent status.
Product Overview
Among organic chlorides, 1-Chlorooctane looks humble, with a single chlorine atom capping a straight eight-carbon chain. It typically appears as a clear, colorless liquid with little odor—though anyone who has handled it directly would agree, "light hydrocarbon" undersells the slightly sharp chemical note that rides along. In everyday workrooms, its main selling point remains the combination of manageable volatility and ready reactivity. Synthetic chemists rely on it for introducing an octyl group. Its price and availability trail its shorter-chain cousins like chlorohexane and chlorobutane, but those working in research or flavor and fragrance precursor manufacture know its value as a building block. Inventory lists show it turns up mostly in specialty shops, not big chemical warehouses.
Physical & Chemical Properties
With a molecular weight above 148 g/mol, 1-Chlorooctane carries more heft than lower chlorinated alkanes. The density lands around 0.88 g/cm3, so it floats a bit on water, but not by much. Its boiling point hovers near 180°C—fairly high for a hydrophobic compound without polar groups besides that lone chlorine. Solubility in water barely registers: less than a gram per liter dissolves. It readily mixes with common organic solvents like ether, benzene, or hexane. The molecule’s chemical character comes mostly from the carbon-chlorine bond. That bond, polar and relatively strong, allows the octyl chain to act as a backbone for substitutions or nucleophilic displacement, especially in laboratory settings. The label on any lab bottle will mention its flammability and call out its volatility, though a person working in a ventilated hood won’t smell much past that faint alkyl tang.
Technical Specifications & Labeling
Quality control labs insist on strict technical parameters for every lot. Purity levels for 1-Chlorooctane usually run at or above 98%, with some vendors pushing “premium” grades above 99%. The usual GC or GC-MS reports back the main organic impurities—typically trace 1-octanol left from synthesis or other octyl halides produced as byproducts. Each drum or bottle comes stamped with a batch number, HS code, hazard symbols, recommended storage conditions (dark, below 25°C, away from incompatible chemicals like strong acids), and a hazard class sticker identifying it under local transport regulations. Standard safety data matches GHS criteria, warning workers to avoid skin or eye contact, and never inhale vapor for long due to its potential irritation.
Preparation Method
To create 1-Chlorooctane at scale, chemical plants use direct chlorination of n-octanol. The typical pathway involves treating the alcohol with thionyl chloride (SOCl2), triphosgene, or phosphorus trichloride under controlled cooling, tossing in a bit of pyridine or DMF as catalyst. The reaction churns out hydrogen chloride or sulfur dioxide as gas byproducts. For small labs, careful fractionation comes next; for big factories, it shifts to industrial column distillation. As someone who’s watched the process firsthand, the application of vacuum lines streamlines the removal of excess starting material, avoids over-chlorination, and cuts the formation of unpleasant secondary or tertiary isomers. Waste stream neutralization, especially for chloride-rich gases, requires precise engineering to satisfy growing safety and emission regulations.
Chemical Reactions & Modifications
Among chain chlorides, 1-Chlorooctane stands out because the terminal halogen makes it a starting point for so many organic modifications. The classic nucleophilic substitution pops up in almost every undergraduate text: throw a nucleophile like sodium cyanide, sodium azide, or an amine at it, and the chlorine swaps out, giving access to octylnitriles, amines, and ethers. It acts as an alkylating agent for building surfactant headgroups, drug molecules, or flavor precursors. Conversion to Grignard reagents opens a route for coupling with aromatic systems. Friedel-Crafts alkylation introduces an octyl group onto aromatic rings, and many flavor compounds or lubrication additives track their roots to simple reactions like these. Synthetic chemists value its selectivity—a gift from the primary carbon-chlorine placement—whereas industrial operators care that its boiling range allows easy fractionation and recovery in multi-step syntheses.
Synonyms & Product Names
Few chemicals carry as many trade monikers as 1-Chlorooctane. Across catalogs and regulatory filings, it answers to names such as n-Octyl chloride, Octyl chloride, 1-chloro-n-octane, and sometimes even under less common designations like Capryl chloride. Laboratories label it per IUPAC as 1-Chlorooctane, but manufacturing sheets sometimes preserve historical quirks, listing it as NCO or simply “chlorooctane” if there’s no confusion with isomeric forms. The safety paperwork almost always leads with the most precise form to avoid confusion with positional or structural isomers.
Safety & Operational Standards
Any chemical with volatility and reactivity demands respect in handling. 1-Chlorooctane brings flammable vapor, and inhalation risks uncommon in less polar alkanes. Storage rooms use only spark-proof fittings, and safety instructions urge users to handle it under strong ventilation. Absorption through skin can happen after prolonged exposure, and anyone familiar with industrial practice insists on full nitrile gloves—PVC ones soften and degrade. Procedures for dealing with spills lean on standard alkyl halide protocols: neutral absorbent pads, sealed waste bins, and quick isolation of vapor. Eye protection goes without saying after one close call in an academic facility where a pipette tip snapped, splashing a worker. Supply chains must keep a close eye on container labels given the risk of commingling with similar-looking but much more hazardous halides like 1-chlorooctadecane.
Application Area
Most outside chemistry have never heard of 1-Chlorooctane, yet its impact quietly spreads across several corners of manufacturing and research. Its chain length fits sweetly as a base for specialty surfactants—especially anti-static agents for polymers, or as intermediates for making quaternary ammonium salts. Flavor and fragrance labs count on it for building rare octyl esters. Lubricant producers sometimes use it for modifying oil additives, extending both viscosity and hydrolytic stability. Crop protection chemistries find value in the long chain for anchoring low-volatility molecules. I’ve even seen the odd report about its use as a model compound in environmental fate studies, gauging how alkyl chlorides behave as pollutants. Its modest production volumes reflect its status as a custom intermediate rather than a bulk commodity.
Research & Development
In academic literature, 1-Chlorooctane rarely headlines studies, but its profile appears frequently in the supporting data for new surfactants, phase transfer catalysts, or in research modeling skin penetration of alkyl halides. Its tractable synthesis and well-understood reactivity keep it in the toolkits of academic and industrial chemists hunting for structure-activity relationships or scaling new organic reactions. Equipment upgrades and safer reagents (replacement of toxic phosphorus chlorides) edge in every decade, always aiming for cleaner yield, waste minimization, and fewer worker exposure risks. Environmental researchers use standards like 1-Chlorooctane as model pollutants, probing how long-chain halides leach through soil or resist breakdown in treatment works—a reminder that every lab procedure eventually feeds into real-world questions about persistence and bioaccumulation. Ongoing innovation in green chemistry keeps nudging the process efficiency forward while lowering emissions and disposal hazards.
Toxicity Research
Toxicologists point to a narrow but growing body of research tracking the effects 1-Chlorooctane can have on humans and wildlife. Acute exposure tends to irritate skin, eyes, and the respiratory tract, while chronic inhalation raises concerns about liver stress or neurotoxicity that mirror trends in similar alkyl chlorides. The molecule resists rapid biodegradation and builds up in fatty tissue, especially in aquatic animals—echoing a larger topic on bioaccumulation of long-chain halocarbons. Laboratory tests on rodents convince safety committees to set handling limits and keep spill contingency plans updated. Data for groundwater contamination remain limited, but regulatory agencies recognize its persistence and monitor industrial use points closely. My own training in chemical safety always called for strict personal protective equipment, even with compounds of “moderate” toxicity—especially where volatility and skin absorption risk overlap.
Future Prospects
The fate of 1-Chlorooctane will ride on evolving chemistry, tighter regulations, and smarter green alternatives. Pressure to cut volatile organic compound emissions and limit release of persistent halogenated molecules pushes researchers and manufacturers alike to rethink chlorinated intermediates. Demand will keep level in specialty synthesis—where no drop-in alternative carries the simplicity and reactivity of the terminal chloride—but will face more scrutiny outside closed-process systems. New catalysis methods and milder chlorination procedures promise safer production with lower waste. In labs that value greener chemistry and process efficiency, alternative reagents may eventually take over some of 1-Chlorooctane’s traditional roles. Its utility in specialized surfactants and structurally precise molecules means it won’t vanish from shelves. Where I’ve worked, the real progress often flows from people on the warehouse floor and in the pilot plants, finding ways to handle it more safely, minimize waste, and trace every milliliter from delivery to final product. Future safety research—especially into low-dose, long-term environmental effects—will shape how society regards this quietly persistent building block in organic synthesis.
A Real-World Perspective on a Niche Organic Chemical
In chemistry labs, bottles labeled with names like 1-Chlorooctane often hide in plain sight, but this clear, sometimes overlooked liquid often plays key roles behind the scenes. At first glance, it looks like many other colorless chemicals. Dig a little deeper, and you’ll see it helps drive some crucial processes in manufacturing, research, and even pharmaceuticals.
1-Chlorooctane: The Basics
The structure of 1-Chlorooctane carries real weight for chemists. You’ve got a straight eight-carbon chain, capped with a chlorine atom. That might not sound fascinating to everyone, but it makes all the difference in labs that need a reliable alkyl halide to start chemical reactions. The presence of chlorine makes the molecule reactive—a perfect launchpad for building bigger and more complex organic molecules.
Making Other Chemicals: Synthesis Matters
In practical terms, 1-Chlorooctane acts as a building block. Chemical companies use it to introduce an octyl group, or an eight-carbon chain, into other molecules. This sounds technical, but here’s an example: imagine designing a new lubricant, surfactant, or specialty plastic. Engineers often reach for 1-Chlorooctane to get precise control over the properties of the final material.
It’s also present in the toolkits of organic chemists who develop medicine. Compounds built up from 1-Chlorooctane end up in early-stage drug candidates. Sometimes, tweaking a single carbon chain length on a molecule changes the way a drug moves through the body. That’s not a theory—drug companies run hundreds of these experiments each year to see which candidate treats disease better or causes fewer side effects.
Laboratory Testing and Academic Research
Academic researchers turn to 1-Chlorooctane when they want to understand fundamental chemistry. Picture a graduate student comparing different alkyl halides to study reaction speed, or tracking what happens when this molecule meets a range of other reactive agents. I remember one lab course where tracking the path from 1-Chlorooctane to a multi-step end product gave everyone a crash course in reaction mechanisms, purification, and chromatography. The lessons stuck.
Industrial Relevance in Everyday Products
Even outside the lab, the impact stretches further than most people realize. Some specialty cleaners, lubricants, and even certain agricultural chemicals use derivatives of 1-Chlorooctane. Its ability to act as an intermediate keeps supply chains running smoothly for many tailored applications. For anyone working in process chemistry, tracing back the raw materials reveals how often a molecule like this stands at a key turning point.
Health, Safety, and Environmental Responsibility
Like any organic halide, safe handling becomes a non-negotiable point. Skin contact and inhalation risks mean that users always need gloves, goggles, and good ventilation. I’ve seen enough lab accidents to know that rushing through these steps never pays off. Industrial users also face stricter rules. Regulations require safe storage and careful disposal to avoid environmental contamination and workplace hazards. Continued vigilance matters, both for personal health and for protecting water and soil ecosystems.
Looking Forward: Greener Alternatives and Safer Practices
Better practices around chemicals like 1-Chlorooctane signal larger shifts in manufacturing. Innovations in “green chemistry” aim to replace chlorine-based reagents with safer, more sustainable solutions. Research continues to find low-impact pathways to the same valuable end products, so the pressure grows for companies and institutions to stay open to change and regularly review safety practices.
Each practical use of 1-Chlorooctane ties back to broader questions about industrial responsibility, laboratory training, and creativity in science. Its significance stretches beyond any single application, highlighting the balance between utility and stewardship in the chemical industry.
Breaking Down the Formula
Anyone peering into an organic chemistry lab or a chemical storage room has come across countless bottles labeled with codes that look like secret shorthand. Spotting "1-Chlorooctane," the mind might not immediately picture eight carbons in a neat chain, topped off by a single chlorine atom. The formula for 1-Chlorooctane is C8H17Cl. It’s straightforward—eight carbons, seventeen hydrogens, and a chlorine tucked at one end of the chain.
Why Structure Matters
Chemistry doesn’t feel distant when real-world uses get involved. With 1-Chlorooctane, structure determines almost everything about its behavior. Chlorine attached to the end carbon gives this compound its reactivity and physical properties. This setup means the molecule won’t shy away from participating in substitution reactions, and its long carbon tail keeps it hydrophobic. Researchers and technicians care about this because the placement of that chlorine has ripple effects in cleaning agents, synthesis for pharmaceuticals, and as steps in making other useful chemicals.
Practical Chemistry in Real Time
During undergraduate lab work, handling compounds like 1-Chlorooctane helped me see the leap from textbook theory to real world. In one lab, coaxing a color change out of a tiny amount of alkyl halide felt more meaningful than any lecture. It’s a recognizable stop in making more sophisticated molecules. Many pharmaceuticals, surfactants, and even agrochemicals start with simple halogenated chains. By dropping the chlorine on the first carbon, chemists build more complexity later on—the “first step” is often the most important one that influences yield and purity downstream.
Safety and Environmental Touchpoints
Handling 1-Chlorooctane means accepting responsibility. It’s not the most toxic compound in the lab, but it’s still an alkyl halide. Historical records show many halogenated hydrocarbons raise concern about cancer risks if not used responsibly. Accidental releases don’t help the environment, as these compounds stick around in soils and waters. Protocols always recommend using gloves and working in a fume hood. Anyone familiar with chemical work knows the mutual respect between human safety and the substance itself. Authorities like the CDC and NIH warn people about inhalation and skin exposure. Those cautions aren’t just red tape—they prevent lasting health trouble.
Paths for Better Practice and Safer Chemistry
Some modern firms already look for green chemistry alternatives, aiming to swap out persistent halogenated compounds. Industries have begun to shift toward less toxic or more easily degradable molecules wherever possible. Laboratories recycle solvents, reduce waste, and plan syntheses with efficiency in mind. On the education side, college labs now dedicate time to chemical safety, waste handling, and reviewing Material Safety Data Sheets. These practices shape responsible habits before mistakes take a toll on people or the planet.
Connecting Science to Life
Highlighting the chemical formula—C8H17Cl—doesn’t just satisfy a quiz or catalog entry. It shows how structure shapes function, influences safety, and guides better methods for future generations. Small changes at the molecular level echo in human health, industry outcomes, and the wider environment, so each step with chemicals like 1-Chlorooctane asks for precision backed by experience and constant learning.
A Closer Look at 1-Chlorooctane's Hazards
Anyone with a background in organic labs or industrial chemistry knows the long list of substances that make their way onto safety data sheets. 1-Chlorooctane, a colorless liquid with a mild odor, often confuses people outside the chemical field. While it’s not as famous as benzene or formaldehyde, this solvent and intermediate deserves a closer look, especially because it may show up in consumer products and factory settings.
Health Risks Get Serious in the Lab
Working with 1-chlorooctane isn’t like working with table salt. This chemical targets the respiratory system if vapors build up. During grad school, I watched colleagues get careless with organic solvents. Irritation, headaches, dizziness—these hit hardest in stuffy, poorly ventilated spaces. Even minor, short exposures to chlorinated hydrocarbons bring discomfort. Longer, heavier exposure risks much worse symptoms, including potential effects to the liver, kidneys, and nervous system.
Skin contact often happens by accident. It dries out skin quick, leaves it itchy, and some people get chemical burns or blisters when they don’t use gloves. Splashing it in the eyes needs immediate rinsing, which costs precious time in any emergency. That’s not just policy—it’s something I’ve had to do for a lab partner who underestimated “basic” solvents.
No one should assume a “mild” chemical is safe just because it isn’t listed as a known carcinogen or banned outright. 1-Chlorooctane hasn’t been studied as deeply as other chlorinated hydrocarbons, but that gap in research is no comfort. Lack of long-term human data doesn’t mean no risk, only less clarity.
These Molecules Hang Around in the Environment
Chemicals like 1-chlorooctane don’t disappear when poured down a drain or left on rags. The carbon-chlorine bond in the molecule resists breakdown. If this solvent leaks into groundwater, it sticks around, potentially reaching drinking supplies. I’ve read real-life examples from sites near old chemical plants; even if contamination seems minor at first, chlorinated pollutants often show up years later, usually in wells or surface water.
In my environmental consulting days, we spent months sampling soils near storage tanks and drum sites. 1-Chlorooctane counts as a volatile organic compound (VOC), so it travels in air and water. VOCs add up to form smog and indirectly impact public health. Aquatic life rarely deals well with these substances, which bioaccumulate and can harm sensitive species—including the ones humans rely on for food.
Reducing the Risks
The answer isn’t to panic, but to respect the protocols. Chemical fume hoods, gloves, goggles, closed containers—every part of the basic “lab PPE” list matters, even with obscure chemicals. Most problems I saw over years in research or industry came not from the chemicals themselves, but shortcuts and missing training. Those who store or use 1-chlorooctane can cut down on spills with regular leak checks, use proper disposal methods, and follow local regulations.
Substituting less-harmful alternatives for chlorinated solvents works well in many industrial settings. Researchers should push for greener processes and green chemistry solutions, which means rethinking basic materials, not just hiding them behind safety warnings. Most people don't talk about what happens to waste after it leaves the building, but responsibility doesn’t end at the door.
Taking Chemical Safety Personally
1-Chlorooctane doesn’t show up on news feeds every day, but it sits on shelves in plenty of labs and warehouses. Anyone who has worked in a lab or on an industrial site knows that overlooking basic chemical safety can turn a routine day upside down. 1-Chlorooctane brings its own challenges, and because it’s a flammable, volatile, and potentially hazardous liquid, it doesn’t offer second chances. Trouble often begins with shortcuts—like storing chemical drums too close to heaters or ignoring faded hazard labels.
Key Risks: Why Carelessness Has Consequences
This chemical evaporates quickly, releasing vapors that can form explosive mixtures with air. I remember the time a leaky container released enough fume to trigger an alarm across the lab. Thankfully, the ventilation system caught it, but the scent lingered for hours. Accidental contact can irritate skin and eyes, and inhaling fumes doesn’t do lungs any favors. Experience shows spills spread fast on concrete floors, turning a small mishap into a spreading hazard.
Storing it Right: Steps that Save Lives
Metal safety cabinets designed for flammable liquids keep risks in check. Never stack 1-Chlorooctane near oxidizers, acids, or heat sources like radiators or direct sunlight. If you’ve seen melted plastic jugs crumpling under old grow lamps, you know how quickly heat undermines safety. Space matters. Overcrowded shelves lead to accidental bumps and spills, especially when containers sweat in humid weather.
Label every single bottle and drum. Faded marker or torn tape isn’t enough. Clear labels with hazard signs don’t just follow regulations—people read them, especially in emergencies. I’ve had my share of bottle mix-ups and know how a missing tag can trigger a panic during an inspection.
Handling: Strong Habits Make a Difference
Solid gloves—nitrile or neoprene—keep the stuff off your skin. Safety goggles with side shields block sudden splashes. In busy labs, I always reached for face shields during transfers, especially after one splash sent me straight to the eyewash station. Open bottles only in well-ventilated rooms, close to fume hoods. Chemical vapors move fast—windows and simple fans rarely clear the air fast enough.
Never pipette this liquid by mouth, and swap open-flame Bunsen burners for safer heat sources. Fire blankets and extinguishers should sit within arm’s reach, not buried behind stacks of old boxes. People forget they only have seconds to act once a spill ignites.
Waste and Emergency Planning: No Room for Lucky Breaks
Store waste separately in strong, compatible containers with secure lids. Back in the day, careless disposal turns up as odd-smelling stains under benches that nobody claims. One day, there’s no harm; the next, fumes trigger headaches and dizziness across the room. Locked, labeled waste bins and a clear emergency exit path cut through the confusion during a spill.
Building a Culture of Safety
No single guideline beats shared vigilance. Training goes beyond tired PowerPoint slides—it’s about walking people through real scenarios. I’ve seen seasoned techs spot forgotten spills faster than cameras can record. Regular drills, up-to-date Material Safety Data Sheets on every chemical, and simple checklists make good habits automatic.
Storing and handling 1-Chlorooctane isn’t about ticking boxes. It’s about respecting the risks and trusting that safe habits keep everyone around the bench or in the warehouse out of harm’s way.
A Glimpse at Its Appearance
Folks in laboratories and chemical plants spot 1-chlorooctane as a colorless, oily liquid. Unlike some solvents that hit your nose hard, its aroma is faint but still noticeable. This makes handling fairly straightforward, but gloves should always be part of the routine. The substance looks much like many other light hydrocarbons, clear and with no cloudiness or odd tints. If anything turns up murky or off-color, suspicion about contamination or degradation hits right away. Experience tells that packaging matters here—sunlight or reactive containers cause changes in purity, muddying that clean, see-through appearance.
Melting and Boiling Points: Insights From the Lab Bench
1-Chlorooctane has a melting point around -56°C. That's plenty cold—well below most freezers or lab chillers. There’s no solid chunk of this compound forming unless the storage conditions match Antarctic extremes. In practical settings, this property means no worries about it crystallizing during regular transport or winter storage. Out in the field or shipping warehouses, this keeps processes efficient and mishaps minimal.
Boiling sets in near 191°C, higher than you’d expect for a simple alkane thanks to that chlorine tag on the molecule. The reason behind this lies in the increased molecular weight and stronger intermolecular force from chlorine’s electronegativity. Working in distillation, you can depend on this boiling threshold for separating out 1-chlorooctane from lighter by-products—a step I’ve seen trip up newcomers counting on it vaporizing too soon. Rushing the process below 191°C just burns time and resources.
What Science Says About Its Stability
Stability matters for storage and safety, both in professional setups and teaching labs. 1-Chlorooctane keeps its composition when it’s sealed off from air and kept away from strong heat or sunlight. Inside a closed amber bottle tucked in a ventilated cabinet, you won’t see it breaking down anytime soon. This mirrors a big lesson—minimize exposure to oxygen and you stall unwanted reactions. In real work, folks get this wrong when relabeling or swapping containers, leading to headaches when purity testing returns odd figures.
Why Physical Properties Matter in Real Use
Chemists rely on boiling and melting data to plan syntheses, purifications, and safe handling. For 1-chlorooctane, the relatively low melting point means it’s always in liquid form for blending, measuring, or transferring. That ease goes away for some chlorinated compounds that need delicate warming just to pour. Proper knowledge lets users set up distillation columns with the right heat gradient, cutting down energy on unneeded preheating. It also means knowing not to store containers anywhere near sources exceeding 191°C—an uncommon situation in most labs, but not unheard of in facilities that handle lots of volatile materials.
Lessons from mishaps, both mine and others’, show that knowing these numbers is about more than hitting targets in paperwork. One spill from a container left too close to a heat vent demonstrated just how an innocent mistake could escalate into a costly mess. Insurance and clean-up teams spend hours sorting out residues that cling to surfaces due to the oily nature of 1-chlorooctane.
Moving Safety and Quality Forward
Improving safety calls for clear labeling, regular equipment checks for leaks, and ongoing education about actual boiling and melting numbers. Too often newcomers rely on quick reference cards that round off values or miss context, leading to errors. Industry and academia both benefit from better training and closer adherence to true measured figures, not just ballpark estimates. It’s not about memorizing numbers for the sake of it—it’s about keeping workplaces safer, cleaner, and more dependable for everyone involved.
| Names | |
| Preferred IUPAC name | 1-chlorooctane |
| Other names |
n-Octyl chloride
Octyl chloride Chlorooctane 1-Chlorooctyl |
| Pronunciation | /ˈklɔːroʊ.ɒk.teɪn/ |
| Identifiers | |
| CAS Number | 111-85-3 |
| 3D model (JSmol) | `JSmol('load $1-chlorooctane')` |
| Beilstein Reference | 1718735 |
| ChEBI | CHEBI:34399 |
| ChEMBL | CHEMBL15452 |
| ChemSpider | 14174 |
| DrugBank | DB14015 |
| ECHA InfoCard | ECHA InfoCard: 100.007.942 |
| EC Number | 203-876-6 |
| Gmelin Reference | 806706 |
| KEGG | C01780 |
| MeSH | D002643 |
| PubChem CID | 12471 |
| RTECS number | RN0875000 |
| UNII | 2PZ3TMB8GL |
| UN number | UN1992 |
| Properties | |
| Chemical formula | C8H17Cl |
| Molar mass | 162.71 g/mol |
| Appearance | Colourless liquid |
| Odor | Mild odor |
| Density | 0.83 g/mL at 25 °C(lit.) |
| Solubility in water | Insoluble |
| log P | 4.85 |
| Vapor pressure | 3.32 mmHg (at 25 °C) |
| Acidity (pKa) | pKa ≈ 50 |
| Basicity (pKb) | > 15.0 |
| Magnetic susceptibility (χ) | -7.72e-6 cm³/mol |
| Refractive index (nD) | 1.4210 |
| Viscosity | 2.918 mPa·s (25°C) |
| Dipole moment | 1.70 D |
| Thermochemistry | |
| Std molar entropy (S⦵298) | 400.7 J·mol⁻¹·K⁻¹ |
| Std enthalpy of formation (ΔfH⦵298) | -179.6 kJ/mol |
| Std enthalpy of combustion (ΔcH⦵298) | -5347.7 kJ/mol |
| Hazards | |
| GHS labelling | GHS02, GHS07 |
| Pictograms | GHS02, GHS07 |
| Signal word | Warning |
| Hazard statements | H226, H304, H315, H319, H335, H411 |
| Precautionary statements | Precautionary statements of 1-Chlorooctane are: "P210, P233, P240, P241, P242, P243, P261, P264, P271, P301+P310, P303+P361+P353, P304+P340, P305+P351+P338, P312, P332+P313, P337+P313, P362+P364, P370+P378, P403+P235, P501 |
| NFPA 704 (fire diamond) | 1-1-0 |
| Flash point | 85 °C |
| Autoignition temperature | 175 °C |
| Explosive limits | Explosive limits: 0.7–5.6% |
| Lethal dose or concentration | LD50 oral rat 3730 mg/kg |
| LD50 (median dose) | LD50 (median dose): Oral rat 6,230 mg/kg |
| NIOSH | SN2975000 |
| PEL (Permissible) | PEL (Permissible Exposure Limit) of 1-Chlorooctane: Not established |
| REL (Recommended) | REL (Recommended) for 1-Chlorooctane: 1 ppm (6 mg/m³) |
| IDLH (Immediate danger) | Unknown |
| Related compounds | |
| Related compounds |
1-Bromooctane
1-Iodooctane 1-Fluorooctane 1-Chlorononane 1-Chloroheptane |
